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Chapter 10: Q1TY (page 218)

Find the pH of $0.002 {MK}^{+} {HP}^{-}$ with Equation $10 - 11$ .

Short Answer

Expert verified

The pH of given $K^{+} HP'$ solution is 4.28.

Step by step solution

01

Concept used.

Intermediate form of diprotic acid

$[H +] = \sqrt{\frac{K_{1} K_{2} I^{+} + K_{1} K_{w}}{K_{1} + F *}}$

02

Step2: Calculate the pH of 0.002MK+HP-.

The pH,

$[H +] = \sqrt{\frac{(4.7 \times 10^{- 3}) (1.8 \times 10^{- 10}) (0.002) + (4.7 \times 10^{- 3}) (1.0 \times 10^{- 14})}{(4.7 \times 10^{- 3}) + (0.002)}} pH = - \log [H^{+}] = 4.28$

The pH of $K^{+} HP'$ solution is 4.28.

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Most popular questions from this chapter

(a) Calculate the quotient in $[H_{3} {PO}_{4}] / [H_{3} {PO}^{-}_{4}] in 0.0500 M {KH}_{2} {PH}_{4}$ .

(b) Find the same quotient for $0.0500 {MK}_{2} {PO}_{4}$ .

What volume of KOH would bring the pH to 4.50?

The both $^{[H_{2} A] = [H A^{‐}]}$ are equal as found to be $^{pH = 10.54}$

Draw the structures of the predominant forms of glutamic acid and tyrosine at $pH 9.0$ and $pH 10.0$ What is the second most abundant species at each ?.

The base B has $^{{pK}_{b}}$ = 5.00.

(a) What is the value of $^{{pK}_{a}}$ for the acid $^{{BH}^{+}}$ ?

(b) At what pH is [ $^{{BH}^{+}}$ ] = [B]?

(c) Which is the principal species at pH 7.00: B or $^{{BH}^{+}}$ ?

(d) What is the quotient [B] / [ $^{{BH}^{+}}$ ] at pH 12.00?

See all solutions

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