Solution Found!
Calculate the pH of each solution:(a) 0.0155 M HBr(b) 1.28 × 10?3 M KOH(c) 1.89 × 10?3 M
Chapter 14, Problem 77P(choose chapter or problem)
Calculate the pH of each solution:
(a) 0.0155 M HBr
(b) \(\mathrm{1.28 \times 10^{-3}~ M~ KOH}\)
(c) \(\mathrm{1.89 \times 10^{-3}~ M~ HNO_3}\)
(d) \(\mathrm{1.54 \times 10^{-4}~ M~ Sr(OH)_2}\)
Equation Transcription:
Text Transcription:
1.28 x 10^{-3} M KOH
1.89 x 10^{-3} M HNO_3
1.54 x 10^{-4} M Sr(OH)_2
Questions & Answers
QUESTION:
Calculate the pH of each solution:
(a) 0.0155 M HBr
(b) \(\mathrm{1.28 \times 10^{-3}~ M~ KOH}\)
(c) \(\mathrm{1.89 \times 10^{-3}~ M~ HNO_3}\)
(d) \(\mathrm{1.54 \times 10^{-4}~ M~ Sr(OH)_2}\)
Equation Transcription:
Text Transcription:
1.28 x 10^{-3} M KOH
1.89 x 10^{-3} M HNO_3
1.54 x 10^{-4} M Sr(OH)_2
ANSWER:
Solution:
We have to calculate the pH of each solution
Step 1
(a) 0.0155 M HBr
pH is defined as the negative log of hydrogen or hydronium ion concentration.
pH = - log[H+ ]
pH = - log[H+]
= - log (0.0155)
= - (-1.809)
= 1.809
Thus pH of 0.0155 M HBr is 1.809.