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Calculate the pH during the titration of 30,00 mL of
Chapter 20, Problem 40P(choose chapter or problem)
Problem 40P
Calculate the pH during the titration of 30,00 mL of 0.1000 M KOH with 0.1000 M HBr solution after the following additions of acid:
(a) 0 mL
(b) 15.00 mL
(c) 29.00 mL
(d) 29.90 mL
(e) 30.00 mL
(f) 30.10 mL
(g) 40.00 mL
Questions & Answers
QUESTION:
Problem 40P
Calculate the pH during the titration of 30,00 mL of 0.1000 M KOH with 0.1000 M HBr solution after the following additions of acid:
(a) 0 mL
(b) 15.00 mL
(c) 29.00 mL
(d) 29.90 mL
(e) 30.00 mL
(f) 30.10 mL
(g) 40.00 mL
ANSWER:
Step 1 of 8
The Addition of an acid in a base is called a neutralization reaction that gives salt and water as the products.
An equal number of moles of hydrogen and hydroxide ions is required for complete neutralization and the remaining number of ions after the neutralization determines the pH.
The product of the molar concentration and the volume gives us the number of moles as per the formula of molarity.
The reaction between hydrobromic acid and potassium hydroxide takes place as:
Since both the reactants are strong electrolytes, they dissociate completely into their ions and the concentration of HBr or KOH is considered for the calculation of pH.