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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

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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

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.

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