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Chapter 14: QCYL (page 774)

The hydronium ion concentration of vinegar is approximately 4×10−3 M. What are the corresponding values of pOH and pH?

Short Answer

Expert verified

pH can be defined as negative logarithm of H+ ion concentration.\(pOH\;\)can be defined as negative logarithm of hydroxyl ion concentration.

\(\begin{array}{l}pH\; = \; - \log \;{H^ + }\\pOH\; = \; - \log O{H^ - }\end{array}\)

Step by step solution

01

Step-by-step-solution

Hydronium ion concentration can be given as following

02

pH and pOH

\(\begin{array}{c}\left[ {{H_3}{O^ + }} \right] = 4 \times 1{0^{ - 3}}M\\pH = - log\left[ {{H_3}{0^ + }} \right]\\ = - log\left( {4 \times 1{0^{ - 3}}} \right)\\ = - log4 - log\left( {1{0^{ - 3}}} \right)\\ = - log4 + 3\\ = - 0.602 + 3\\ = 2.398\\pH \approx 2.4\\pOH + pH = 14\\pOH = 14 - pH = 14 - 2.4\end{array}\)

\(pOH = 11.6\)

03

Final answer

pH= 2.4

pOH= 11.6

Thus, the values of pH and pOH is sorted out.

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Most popular questions from this chapter

The hydronium ion concentration in a sample of rainwater is found to be \(1.7 \times 1{0^{ - 6}}M\) times 25oC. What is the concentration of hydroxide ions in the rainwater?

Determine whether aqueous solutions of the following salts are acidic, basic, or neutral:

\((a) FeC{l_3}\)

\((b) {K_2}C{O_3}\)

\((c) N{H_4}Br\)

\((d) KCl{O_4}\)

From the equilibrium concentrations given, calculate for each of the weak acids and for each of the weak bases.

\(\begin{aligned}(a)C{H_3}C{O_2}H:\left( {{H_3}{O^ + }} \right) = 1.34 \times 1{0^{ - 3}}M;\left( {C{H_3}CO_2^ - } \right) = 1.34 \times 1{0^{ - 3}}M;\left( {C{H_3}C{O_2}H} \right) = 9.866 \times 1{0^{ - 2}}M;\\(b)Cl{O^ - }:\left( {O{H^ - }} \right) = 4.0 \times 1{0^{ - 4}}M;(HClO) = 2.38 \times 1{0^{ - 5}}M;\left( {Cl{O^ - }} \right) = 0.273M;\\(c)HC{O_2}H:\left( {HC{O_2}H} \right) = 0.524M;\left( {{H_3}{O^ + }} \right) = 9.8 \times 1{0^{ - 3}}M\left( {HCO_2^ - } \right) = 9.8 \times 1{0^{ - 3}}M;\\(d){C_6}{H_5}NH_3^ + :\left( {{C_6}{H_5}NH_3^ + } \right) = 0.233M;\left( {{C_6}{H_5}N{H_2}} \right) = 2.3 \times 1{0^{ - 3}}M;\left( {{H_3}{O^ + }} \right) = 2.3 \times 1{0^{ - 3}}M\end{aligned}\)

From the equilibrium concentrations given, calculate \({K_a}\)for each of the weak acids and \({K_b}\)for each of the weak bases.

\(\begin{aligned}(a)N{H_3}:\left( {O{H^ - }} \right) = 3.1 \times 1{0^{ - 3}}M\left( {NH_4^ + } \right) = 3.1 \times 1{0^{ - 3}}M;\left( {N{H_3}} \right) = 0.533M;\\(b)HN{O_2}:\left( {{H_3}{O^ + }} \right) = 0.011M;\left( {NO_2^ - } \right) = 0.0438M;\left( {HN{O_2}} \right) = 1.07M;\\(c){\left( {C{H_3}} \right)_3}\;N:\left( {{{\left( {C{H_3}} \right)}_3}\;N} \right) = 0.25M;\left( {{{\left( {C{H_3}} \right)}_3}N{H^ + }} \right) = 4.3 \times 1{0^{ - 3}}M;\left( {O{H^ - }} \right) = 4.3 \times 1{0^{ - 3}}M;\\(d)N{H_4} + :\left( {N{H_4} + } \right) = 0.100M;\left( {N{H_3}} \right) = 7.5 \times 1{0^{ - 6}}M;\left( {{H_3}{O^ + }} \right) = 7.5 \times 1{0^{ - 6}}M\end{aligned}\)

\(\begin{aligned}\left( {N{H_3}} \right) = 7.5 \times 1{0^{ - 6}}M\\\left( {{H_3}{O^ + }} \right) = 7.5 \times 1{0^{ - 6}}M\end{aligned}\)

Gastric juice, the digestive fluid produced in the stomach, contains hydrochloric acid, and HCl. Milk of Magnesia, a suspension of solid Mg(OH)2 in an aqueous medium, is sometimes used to neutralize excess stomach acid. Write a complete balanced equation for the neutralization reaction, and identify the conjugate acid-base pairs
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