Find the pH and percent ionization of a 0.100 M solution of a weak monoprotic acid

What causes heartburn? What are some possible ways to alleviate heartburn?

What are the general physical and chemical properties of acids? Of bases?

What is a carboxylic acid? Give an example.

What is the Arrhenius definition of an acid? Of a base?

What is a hydronium ion? Does H+ exist in solution by itself?

What is the BrnstedLowry definition of an acid? Of a base?

Why is there more than one definition of acidbase behavior? Which definition is the right one?

Describe amphoteric behavior and give an example.

What is a conjugate acidbase pair? Provide an example.

Explain the difference between a strong acid and a weak acid and list one example of each.

What are diprotic and triprotic acids? List an example of each.

Define the acid ionization constant and explain its significance.

Write an equation for the autoionization of water and an expression for the ion product constant for water (Kw). What is the value of Kw at 25 C?

What happens to the [OH-] of a solution when the [H3O+] is increased? Decreased?

Define pH. What pH range is considered acidic? Basic? Neutral?

Define pOH. What pOH range is considered acidic? Basic? Neutral?

In most solutions containing a strong or weak acid, the autoionization of water can be neglected when calculating [H3O+]. Explain why this statement is valid.

When calculating [H3O+] for weak acid solutions, we can often use the x is small approximation. Explain the nature of this approximation and why it is valid.

What is the percent ionization of an acid? Explain what happens to the percent ionization of a weak acid as a function of the concentration of the weak acid solution.

In calculating [H3O+] for a mixture of a strong acid and weak acid, the weak acid can often be neglected. Explain why this statement is valid.

Write a generic equation showing how a weak base ionizes water.

How can you determine if an anion will act as a weak base? Write a generic equation showing the reaction by which an anion, A-, acts as a weak base.

What is the relationship between the acid ionization constant for a weak acid ( Ka ) and the base ionization constant for its conjugate base ( Kb )?

What kinds of cations act as weak acids? List some examples.

When calculating the [H3O+] for a polyprotic acid, the second ionization step can often be neglected. Explain why this statement is valid.

For a weak diprotic acid H2X, what is the relationship between [X2-] and Ka2 ? Under what conditions does this relationship exist?

For a binary acid, HiY, which factors affect the relative ease with which the acid ionizes?

Which factors affect the relative acidity of an oxyacid?

What is the Lewis definition of an acid? Of a base?

What is a general characteristic of a Lewis acid? Of a Lewis base?

What is acid rain? What causes it and where is the problem the greatest?

What are the main detrimental effects of acid rain? What is being done to address the problem of acid rain?

Identify each substance as an acid or a base and write a chemical equation showing how it is an acid or a base according to the Arrhenius definition. a. HNO3(aq) b. NH4 +(aq) c. KOH( aq ) d. HC2H3O2(aq)

Identify each substance as an acid or a base and write a chemical equation showing how it is an acid or a base according to the Arrhenius definition. a. HNO3(aq) b. NH4 +(aq) c. KOH( aq ) d. HC2H3O2(aq)

In each reaction, identify the BrnstedLowry acid, the Brnsted Lowry base, the conjugate acid, and the conjugate base. a. H2CO3(aq) + H2O(l) m H3O+(aq) + HCO3 -(aq) b. NH3(aq) + H2O(l) m NH4 +(aq) + OH-(aq) c. HNO3(aq) + H2O(l) h H3O+(aq) + NO3 -(aq) d. C5H5N(aq) + H2O(l) m C5H5NH+(aq) + OH-(aq)

In each reaction, identify the BrnstedLowry acid, the BrnstedLowry base, the conjugate acid, and the conjugate base. a. HI(aq) + H2O(l) h H3O+(aq) + I -(aq) b. CH3NH2(aq) + H2O(l) m CH3NH3 +(aq) + OH-(aq) c. CO3 2-(aq) + H2O(l) m HCO3 -(aq) + OH-(aq) d. HBr(aq) + H2O(l) h H3O+(aq) + Br-(aq)

Write the formula for the conjugate base of each acid. a. HCl b. H2SO3 c. HCHO2 d. HF

Write the formula for the conjugate acid of each base. a. NH3 b. ClO4 - c. HSO4 - d. CO3 2-

Both H2O and H2PO4 - are amphoteric. Write an equation to show how each substance can act as an acid and another equation to show how each can act as a base.

Both HCO3 - and HS- are amphoteric. Write an equation to show how each substance can act as an acid and another equation to show how each can act as a base.

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant ( Ka ). a. HNO3 b. HCl c. HBr d. H2SO3

Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant ( Ka ). a. HF b. HCHO2 c. H2SO4 d. H2CO3

The three diagrams represent three different solutions of the binary acid HA. Water molecules have been omitted for clarity and hydronium ions ( H3O+ ) are represented by hydrogen ions ( H+ ). Rank the acids in order of decreasing acid strength.

Rank the solutions in order of decreasing [H3O+]: 0.10 M HCl; 0.10 M HF; 0.10 M HClO; 0.10 M HC6H5O.

Pick the stronger base from each pair. a. F- or Cl- b. NO2 - or NO3 - c. F- or ClO

Pick the stronger base from each pair. a. ClO4 - or ClO2 - b. Cl- or H2O c. CN- or ClO

Calculate [OH-] in each aqueous solution at 25 C, and classify the solution as acidic or basic. a. [H3O+] = 1.2 * 10-8 M b. [H3O+] = 8.5 * 10-5 M c. [H3O+] = 3.5 * 10-2 M

Calculate [H3O+] in each aqueous solution at 25 C, and classify each solution as acidic or basic. a. [OH-] = 1.1 * 10-9 M b. [OH-] = 2.9 * 10-2 M c. [OH-] = 6.9 * 10-12 M

Calculate the pH and pOH of each solution. a. [H3O+] = 1.7 * 10-8 M b. [H3O+] = 1.0 * 10-7 M c. [H3O+] = 2.2 * 10-6 M

Calculate [H3O+] and [OH-] for each solution. a. pH = 8.55 b. pH = 11.23 c. pH = 2.87

Complete the table. (All solutions are at 25 C. )

Complete the table. (All solutions are at 25 C. )

Like all equilibrium constants, the value of Kw depends on temperature. At body temperature (37 C) , Kw = 2.4 * 10-14. What are the [H3O+] and pH of pure water at body temperature?

The value of Kw increases with increasing temperature. Is the autoionization of water endothermic or exothermic?

Calculate the pH of each acid solution. Explain how the resulting pH values demonstrate that the pH of an acid solution should carry as many digits to the right of the decimal place as the number of significant figures in the concentration of the solution. [H 3 O + ] = 0.044 M [H 3 O + ] = 0.045 M [H 3 O + ] = 0.046 M

Determine the concentration of H 3 O + to the correct number of significant figures in a solution with each pH. Describe how these calculations show the relationship between the number of digits to the right of the decimal place in pH and the number of significant figures in concentration. pH = 2.50 pH = 2.51 pH = 2.52

Determine the concentration of H 3 O + to the correct number of significant figures in a solution with each pH. Describe how these calculations show the relationship between the number of digits to the right of the decimal place in pH and the number of significant figures in concentration. pH = 2.50 pH = 2.51 pH = 2.52

Determine the pH of each solution. a. 0.048 M HI b. 0.0895 M HClO4 c. a solution that is 0.045 M in HClO4 and 0.048 M in HCl d. a solution that is 1.09% HCl by mass (assume a density of 1.01 g>mL for the solution)

What mass of HI should be present in 0.250 L of solution to obtain a solution with each pH value? a. pH = 1.25 b. pH = 1.75 c. pH = 2.85

What mass of HClO4 should be present in 0.500 L of solution to obtain a solution with each pH value? a. pH = 2.50 b. pH = 1.50 c. pH = 0.50

What is the pH of a solution in which 224 mL of HCl( g ), measured at 27.2 C and 1.02 atm, is dissolved in 1.5 L of aqueous solution?

What volume of a concentrated HCl solution, which is 36.0% HCl by mass and has a density of 1.179 g>mL, should be used to make 5.00 L of an HCl solution with a pH of 1.8?

Determine the [H3O+] and pH of a 0.100 M solution of benzoic acid.

Determine the [H3O+] and pH of a 0.200 M solution of formic acid.

Determine the pH of an HNO2 solution of each concentration. In which cases can you not make the simplifying assumption that x is small ? a. 0.500 M b. 0.100 M c. 0.0100 M

Determine the pH of an HF solution of each concentration. In which cases can you not make the simplifying assumption that x is small ? a. 0.250 M b. 0.0500 M c. 0.0250 M

If 15.0 mL of glacial acetic acid (pure HC2H3O2) is diluted to 1.50 L with water, what is the pH of the resulting solution? The density of glacial acetic acid is 1.05 g>mL.

Calculate the pH of a formic acid solution that contains 1.35% formic acid by mass. (Assume a density of 1.01 g>mL for the solution.)

A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calculate the acid ionization constant (Ka) for the acid.

A 0.115 M solution of a weak acid (HA) has a pH of 3.29. Calculate the acid ionization constant (Ka) for the acid.

Determine the percent ionization of a 0.125 M HCN solution.

Determine the percent ionization of a 0.225 M solution of benzoic acid.

Calculate the percent ionization of an acetic acid solution having the given concentration. a. 1.00 M b. 0.500 M c. 0.100 M d. 0.0500 M

Calculate the percent ionization of a formic acid solution having the given concentration. a. 1.00 M b. 0.500 M c. 0.100 M d. 0.0500 M

A 0.148 M solution of a monoprotic acid has a percent ionization of 1.55%. Determine the acid ionization constant (Ka) for the acid.

A 0.085 M solution of a monoprotic acid has a percent ionization of 0.59%. Determine the acid ionization constant (Ka) for the acid.

Find the pH and percent ionization of each HF solution. a. 0.250 M HF b. 0.100 M HF c. 0.050 M HF

Find the pH and percent ionization of a 0.100 M solution of a weak monoprotic acid having the given \(K_{\mathrm{a}}\) values. a. \(K_{\mathrm{a}}=1.0 \times 10^{-5}\) b. \(K_{\mathrm{a}}=1.0 \times 10^{-3}\) c. \(K_{\mathrm{a}}=1.0 \times 10^{-1}\)

Find the pH of each mixture of acids. a. 0.115 M in HBr and 0.125 M in HCHO2 b. 0.150 M in HNO2 and 0.085 M in HNO3 c. 0.185 M in HCHO2 and 0.225 M in HC2H3O2 d. 0.050 M in acetic acid and 0.050 M in hydrocyanic acid

Find the pH of each mixture of acids. a. 0.075 M in HNO3 and 0.175 M in HC7H5O2 b. 0.020 M in HBr and 0.015 M in HClO4 c. 0.095 M in HF and 0.225 M in HC6H5O d. 0.100 M in formic acid and 0.050 M in hypochlorous acid

For each strong base solution, determine [OH-], [H3O+], pH, and pOH. a. 0.15 M NaOH b. 1.5 * 10-3 M Ca(OH)2 c. 4.8 * 10-4 M Sr(OH)2 d. 8.7 * 10-5 M KOH

For each strong base solution, determine [OH-], [H3O+], pH, and pOH. a. 8.77 * 10-3 M LiOH b. 0.0112 M Ba(OH)2 c. 1.9 * 10-4 M KOH d. 5.0 * 10-4 M Ca(OH)2

Determine the pH of a solution that is 3.85% KOH by mass. Assume that the solution has density of 1.01 g>mL.

Determine the pH of a solution that is 1.55% NaOH by mass. Assume that the solution has density of 1.01 g>mL.

What volume of 0.855 M KOH solution is required to make 3.55 L of a solution with pH of 12.4?

What volume of a 15.0% by mass NaOH solution, which has a density of 1.116 g>mL, should be used to make 5.00 L of an NaOH solution with a pH of 10.8?

Write equations showing how each weak base ionizes water to form OH-. Also write the corresponding expression for Kb. a. NH3 b. HCO3 - c. CH3NH2

Write equations showing how each weak base ionizes water to form OH-. Also write the corresponding expression for Kb. a. CO3 2- b. C6H5NH2 c. C2H5NH2

Determine the [OH-], pH, and pOH of a 0.15 M ammonia solution.

Determine the [OH-], pH, and pOH of a solution that is 0.125 M in CO3 2-.

Caffeine ( C8H10N4O2 ) is a weak base with a p Kb of 10.4. Calculate the pH of a solution containing a caffeine concentration of 455 mg>L.

Amphetamine ( C9H13N ) is a weak base with a pKb of 4.2. Calculate the pH of a solution containing an amphetamine concentration of 225 mg>L.

Morphine is a weak base. A 0.150 M solution of morphine has a pH of 10.5. What is Kb for morphine?

A 0.135 M solution of a weak base has a pH of 11.23. Determine Kb for the base.

Determine if each anion acts as a weak base in solution. For those anions that are basic, write an equation that shows how the anion acts as a base. a. Br- b. ClO- c. CN- d. Cl

Determine whether each anion is basic or neutral. For those anions that are basic, write an equation that shows how the anion acts as a base. a. C7H5O2 - b. I - c. NO3 - d. F

Determine the [OH-] and pH of a solution that is 0.140 M in F-

Determine the [OH-] and pH of a solution that is 0.250 M in HCO3

Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. a. NH4 + b. Na+ c. Co3+ d. CH2NH3 +

Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. a. Sr2+ b. Mn3+ c. C5H5NH+ d. Li+

Determine if each salt will form a solution that is acidic, basic, or pH-neutral. a. FeCl3 b. NaF c. CaBr2 d. NH4Br e. C6H5NH3NO2

Determine if each salt will form a solution that is acidic, basic, or pH-neutral. a. Al(NO3)3 b. C2H5NH3NO3 c. K2CO3 d. RbI e. NH4ClO

Arrange the solutions in order of increasing acidity. NaCl, NH4Cl, NaHCO3, NH4ClO2, NaOH

Arrange the solutions in order of increasing basicity. CH3NH3Br, KOH, KBr, KCN, C5H5NHNO2

Determine the pH of each solution. a. 0.10 M NH4Cl b. 0.10 M NaC2H3O2 c. 0.10 M NaCl

Determine the pH of each solution. a. 0.20 M KCHO2 b. 0.20 M CH3NH3I c. 0.20 M KI

Calculate the concentration of all species in a 0.15 M KF solution.

Calculate the concentration of all species in a 0.225 M C6H5NH3Cl solution.

Write chemical equations and corresponding equilibrium expressions for each of the three ionization steps of phosphoric acid.

Write chemical equations and corresponding equilibrium expressions for each of the two ionization steps of carbonic acid.

Calculate the [H3O+] and pH of each polyprotic acid solution. a. 0.350 M H3PO4 b. 0.350 M H2C2O4

Calculate the [H3O+] and pH of each polyprotic acid solution. a. 0.125 M H2CO3 b. 0.125 M H3C6H5O7

Calculate the concentration of all species in a 0.500 M solution of H2SO3.

Calculate the concentration of all species in a 0.155 M solution of H2CO3.

Calculate the [H3O+] and pH of each H2SO4 solution. At approximately what concentration does the x is small approximation break down? a. 0.50 M b. 0.10 M c. 0.050 M

Consider a 0.10 M solution of a weak polyprotic acid \(\left(\mathrm{H}_2\mathrm{A}\right)\) with the possible values of \(K_{\mathrm{a}_{1}}\) and \(K_{\mathrm{a}_{2}}\) given here. a. \(K_{\mathrm{a}_1}=1.0\times10^{-4};\ K_{\mathrm{a}_2}=5.0\times10^{-5}\) b. \(K_{\mathrm{a}_1}=1.0\times10^{-4};\ K_{\mathrm{a}_2}=1.0\times10^{-5}\) c. \(K_{\mathrm{a}_1}=1.0\times10^{-4};\ K_{\mathrm{a}_2}=1.0\times10^{-6}\) Calculate the contributions to \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) from each ionization step. At what point can the contribution of the second step be neglected?

Based on their molecular structure, pick the stronger acid from each pair of binary acids. Explain your choice. a. HF and HCl b. H2O or HF c. H2Se or H2S

Based on molecular structure, arrange the binary compounds in order of increasing acid strength. Explain your choice. H2Te, HI, H2S, NaH

Based on their molecular structure, pick the stronger acid from each pair of oxyacids. Explain your choice. a. H2SO4 or H2SO3 b. HClO2 or HClO c. HClO or HBrO d. CCl3COOH or CH3COOH

Based on molecular structure, arrange the oxyacids in order of increasing acid strength. Explain your choice. HClO3, HIO3, HBrO3

Which is a stronger base, S2- or Se2-? Explain.

Which is a stronger base, PO4 3- or AsO4 3-? Explain.

Classify each species as either a Lewis acid or a Lewis base. a. Fe3+ b. BH3 c. NH3 d. F

Classify each species as either a Lewis acid or a Lewis base. a. BeCl2 b. OHc. B(OH)3 d. CN

Identify the Lewis acid and Lewis base from among the reactants in each equation. a. Fe3+(aq) + 6 H2O(l) m Fe(H2O)6 3+(aq) b. Zn2+(aq) + 4 NH3(aq) m Zn(NH3)4 2+(aq) c. (CH3)3N(g) + BF3(g) m (CH3)3NBF3(s)

Identify the Lewis acid and Lewis base from among the reactants in each equation. a. Ag+(aq) + 2 NH3(aq) m Ag(NH3)2 +(aq) b. AlBr3 + NH3 m H3NAlBr3 c. F-(aq) + BF3(aq) m BF4 -(aq)

Based on these molecular views, determine whether each pictured acid is weak or strong.

Based on these molecular views, determine whether each pictured base is weak or strong.

The binding of oxygen by hemoglobin in the blood involves the equilibrium reaction: HbH+(aq) + O2(aq) m HbO2(aq) + H+(aq) In this equation, Hb is hemoglobin. The pH of normal human blood is highly controlled within a range of 7.35 to 7.45. Given the above equilibrium, why is this important? What would happen to the oxygen-carrying capacity of hemoglobin if blood became too acidic (a dangerous condition known as acidosis)?

Carbon dioxide dissolves in water according to the equations: CO2(g) + H2O(l) m H2CO3(aq) H2CO3(aq) + H2O(l) m HCO3 -(aq) + H3O+(aq) Carbon dioxide levels in the atmosphere have increased about 20% over the last century. Given that Earths oceans are exposed to atmospheric carbon dioxide, what effect might the increased CO2 have on the pH of the worlds oceans? What effect might this change have on the limestone structures ( primarily CaCO3) of coral reefs and marine shells?

People often take milk of magnesia to reduce the discomfort associated with acid stomach or heartburn. The recommended dose is 1 teaspoon, which contains 4.00 * 102 mg of Mg(OH)2. What volume of an HCl solution with a pH of 1.3 can be neutralized by one dose of milk of magnesia? If the stomach contains 2.00 * 102 mL of pH 1.3 solution, will all the acid be neutralized? If not, what fraction will be neutralized?

Lakes that have been acidified by acid rain can be neutralized by liming, the addition of limestone (CaCO3). How much limestone (in kg) is required to completely neutralize a 4.3 billion liter lake with a pH of 5.5?

Acid rain over the Great Lakes has a pH of about 4.5. Calculate the [H3O+] of this rain and compare that value to the [H3O+] of rain over the West Coast that has a pH of 5.4. How many times more concentrated is the acid in rain over the Great Lakes?

White wines tend to be more acidic than red wines. Find the [H3O+] in a Sauvignon Blanc with a pH of 3.23 and a Cabernet Sauvignon with a pH of 3.64. How many times more acidic is the Sauvignon Blanc?

Common aspirin is acetylsalicylic acid, which has the structure shown here and a pKa of 3.5. C C C C C O O H H H H H H H H C O O C C C Calculate the pH of a solution in which one normal adult dose of aspirin ( 6.5 * 102 mg ) is dissolved in 8.0 ounces of water.

The AIDS drug zalcitabine (also known as ddC) is a weak base with the structure shown here and a pKb of 9.8. H H C C H H H C C O C N N H H H C H C H C H C C O O H O What percentage of the base is protonated in an aqueous zalcitabine solution containing 565 mg>L?

Determine the pH of each solution. a. 0.0100 M HClO4 b. 0.115 M HClO2 c. 0.045 M Sr(OH)2 d. 0.0852 M KCN e. 0.155 M NH4Cl

Determine the pH of each solution. a. 0.0650 M HNO3 b. 0.150 M HNO2 c. 0.0195 M KOH d. 0.245 M CH3NH3I e. 0.318 M KC6H5O

Determine the pH of each two-component solution. a. 0.0550 M in HI and 0.00850 M in HF b. 0.112 M in NaCl and 0.0953 M in KF c. 0.132 M in NH4Cl and 0.150 M HNO3 d. 0.0887 M in sodium benzoate and 0.225 M in potassium bromide e. 0.0450 M in HCl and 0.0225 M in HNO3

Determine the pH of each two-component solution. a. 0.050 M KOH and 0.015 M Ba(OH)2 b. 0.265 M NH4NO3 and 0.102 M HCN c. 0.075 M RbOH and 0.100 M NaHCO3 d. 0.088 M HClO4 and 0.022 M KOH e. 0.115 M NaClO and 0.0500 M KI

Write net ionic equations for the reactions that take place when aqueous solutions of the following substances are mixed: a. sodium cyanide and nitric acid b. ammonium chloride and sodium hydroxide c. sodium cyanide and ammonium bromide d. potassium hydrogen sulfate and lithium acetate e. sodium hypochlorite and ammonia

Morphine has the formula C17H19NO3. It is a base and accepts one proton per molecule. It is isolated from opium. A 0.682 g sample of opium is found to require 8.92 mL of a 0.0116 M solution of sulfuric acid for neutralization. Assuming that morphine is the only acid or base present in opium, calculate the percent morphine in the sample of opium.

The pH of a 1.00 M solution of urea, a weak organic base, is 7.050. Calculate the Ka of protonated urea.

A solution is prepared by dissolving 0.10 mol of acetic acid and 0.10 mol of ammonium chloride in enough water to make 1.0 L of solution. Find the concentration of ammonia in the solution.

Lactic acid is a weak acid found in milk. Its calcium salt is a source of calcium for growing animals. A saturated solution of this salt, which we can represent as Ca(Lact) 2 has a [Ca2+] = 0.26 M and a pH = 8.40. Assuming the salt is completely dissociated, calculate the Ka of lactic acid.

A solution of 0.23 mol of the chloride salt of protonated quinine ( QH+ ), a weak organic base, in 1.0 L of solution has pH = 4.58. Find the Kb of quinine (Q).

A student mistakenly calculates the pH of a 1.0 * 10-7 M HI solution to be 7.0. Explain why the student is incorrect and calculate the correct pH.

When 2.55 g of an unknown weak acid (HA) with a molar mass of 85.0 g>mol is dissolved in 250.0 g of water, the freezing point of the resulting solution is -0.257 C. Calculate Ka for the unknown weak acid.

Calculate the pH of a solution that is 0.00115 M in HCl and 0.0100 M in HClO2.

To what volume should you dilute 1 L of a solution of a weak acid HA to reduce the [H+] to one-half of that in the original solution?

HA, a weak acid, with Ka = 1.0 * 10-8 , also forms the ion HA2 -. The reaction is HA(aq) + A-(aq) m HA2 -(aq) and its K = 4.0. Calculate the [H+], [A-], and [HA2 -] in a 1.0 M solution of HA.

Basicity in the gas phase can be defined as the proton affinity of the base, for example, CH3NH2(g) + H+(g) m CH3NH3 +(g). In the gas phase, (CH3)3N is more basic than CH3NH2 while in solution the reverse is true. Explain this observation.

Calculate the pH of a solution prepared from 0.200 mol of NH 4 CN and enough water to make 1.00 L of solution.

To 1.0 L of a 0.30 M solution of HClO 2 is added 0.20 mol of NaF. Calculate the [HClO 2 ] at equilibrium.

A mixture of Na2CO3 and NaHCO3 has a mass of 82.2 g. It is dissolved in 1.00 L of water and the pH is found to be 9.95. Find the mass of NaHCO 3 in the mixture.

A mixture of Na2CO3 and NaHCO3 has a mass of 82.2 g. It is dissolved in 1.00 L of water and the pH is found to be 9.95. Find the mass of NaHCO 3 in the mixture.

Without doing any calculations, determine which solution in each pair is more acidic. a. 0.0100 M in HCl and 0.0100 M in KOH b. 0.0100 M in HF and 0.0100 M in KBr c. 0.0100 M in NH4Cl and 0.0100 M in CH3NH3Br d. 0.100 M in NaCN and 0.100 M in CaCl2

Without doing any calculations, determine which solution in each pair is more basic. a. 0.100 M in NaClO and 0.100 M in NaF b. 0.0100 M in KCl and 0.0100 M in KClO2 c. 0.0100 M in HNO3 and 0.0100 M in NaOH d. 0.0100 M in NH4Cl and 0.0100 M in HCN

Rank the acids in order of increasing acid strength. CH3COOH CH2ClCOOH CHCl2COOH CCl3COOH