Solution Found!
Calculate the pH of each solution:(a) 1.34 × 10?3 M HClO4(b) 0.0211 M NaOH(c) 0.0109 M
Chapter 14, Problem 78P(choose chapter or problem)
QUESTION:
Calculate the pH of each solution:
(a) \(\mathrm{1.34 \times 10^{-3}~ M~ HClO_4}\)
(b) 0.0211 M NaOH
(c) 0.0109 M HBr
(d) \(\mathrm{7.02 \times 10^{-5}~ M~ Ba(OH)_2}\)
Questions & Answers
QUESTION:
Calculate the pH of each solution:
(a) \(\mathrm{1.34 \times 10^{-3}~ M~ HClO_4}\)
(b) 0.0211 M NaOH
(c) 0.0109 M HBr
(d) \(\mathrm{7.02 \times 10^{-5}~ M~ Ba(OH)_2}\)
ANSWER:Solution 78P:
Here, we are going to calculate the pH of each solution.
pH is defined as the negative log of hydrogen or hydronium ion concentration.
pH = - log[H+ ]
(a) 1.34 × 10−3 M HClO4
We know,
pH = - log[H+]
= - log (1.34 × 10−3 )
= -log 1.34 - log 10−3
= -0.127 +3 = 2.87
Thus, pH of 1.34 × 10−3 M HClO4 is 2.87.
(b) 0.0211 M NaOH
We know,