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Chapter 14: Problem 56

Calculate the \(\mathrm{pH}\) of each of the following solutions containing a strong acid in water. a. \(2.0 \times 10^{-2} \mathrm{M} \mathrm{HNO}_{3}\) c. \(6.2 \times 10^{-12} \mathrm{M} \mathrm{HNO}_{3}\) b. \(4.0 \mathrm{M} \mathrm{HNO}_{3}\)

Short Answer

Expert verified
In conclusion, the pH values of the given HNO3 solutions are: a. 1.70 b. -0.60 c. 11.21

Step by step solution

01

Since HNO3 is a strong acid and fully dissociates in water, the concentration of H+ ions is equal to the concentration of HNO3: \[2.0 \times 10^{-2} \mathrm{M}\]. #Step 2: Calculate the pH#

\(\mathrm{pH} = -\log_{10}[\mathrm{H^{+}}]\), where \([\mathrm{H^{+}}] = 2.0 \times 10^{-2} \mathrm{M}\). Therefore, the pH is approximately 1.70. #b. 4.0 M HNO3# #Step 1: Identify the concentration of H+ ions#
02

Since HNO3 is a strong acid and fully dissociates in water, the concentration of H+ ions is equal to the concentration of HNO3: \[4.0 \mathrm{M}\]. #Step 2: Calculate the pH#

\(\mathrm{pH} = -\log_{10}[\mathrm{H^{+}}]\), where \([\mathrm{H^{+}}] = 4.0 \mathrm{M}\). Therefore, the pH is approximately -0.60. (Note: While the pH is typically expected to be between 0 and 14, strong acid solutions prepared with molar concentrations greater than 1 can result in negative pH values. This indicates that the solution is extremely acidic.) #c. 6.2 x 10^-12 M HNO3# #Step 1: Identify the concentration of H+ ions#
03

Since HNO3 is a strong acid and fully dissociates in water, the concentration of H+ ions is equal to the concentration of HNO3: \[6.2 \times 10^{-12} \mathrm{M}\]. #Step 2: Calculate the pH#

\(\mathrm{pH} = -\log_{10}[\mathrm{H^{+}}]\), where \([\mathrm{H^{+}}] = 6.2 \times 10^{-12} \mathrm{M}\). Therefore, the pH is approximately 11.21. In conclusion, the pH values of the given HNO3 solutions are: a. 1.70 b. -0.60 c. 11.21

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Most popular questions from this chapter

For the following, mix equal volumes of one solution from Group I with one solution from Group II to achieve the indicated \(\mathrm{pH}\). Calculate the \(\mathrm{pH}\) of each solution. Group I: \(0.20 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}, 0.20 \mathrm{MHCl}, 0.20 \mathrm{M} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3} \mathrm{Cl}, 0.20\) \(M\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{3} \mathrm{NHCl}\) Group II: \(0.20 \mathrm{M} \mathrm{KOI}, 0.20 \mathrm{M} \mathrm{NaCN}, 0.20 \mathrm{M} \mathrm{KOCl}, 0.20 \mathrm{M}\) \(\mathrm{NaNO}_{2}\) a. the solution with the lowest \(\mathrm{pH}\) b. the solution with the highest \(\mathrm{pH}\) c. the solution with the \(\mathrm{pH}\) closest to \(7.00\)

At \(25^{\circ} \mathrm{C}\), a saturated solution of benzoic acid \(\left(K_{\mathrm{a}}=6.4 \times 10^{-5}\right)\) has a pH of \(2.80\). Calculate the water solubility of benzoic acid in moles per liter.

Identify the Lewis acid and the Lewis base in each of the following reactions. a. \(\mathrm{B}(\mathrm{OH})_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{B}(\mathrm{OH})_{4}^{-}(a q)+\mathrm{H}^{+}(a q)\) b. \(\mathrm{Ag}^{+}(a q)+2 \mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}(a q)\) c. \(\mathrm{BF}_{3}(g)+\mathrm{F}^{-}(a q) \rightleftharpoons \mathrm{BF}_{4}^{-}(a q)\)

Place the species in each of the following groups in order of increasing base strength. Give your reasoning in each case. a. \(\mathrm{IO}_{3}^{-}, \mathrm{Br} \mathrm{O}_{3}^{-}\) b. \(\mathrm{NO}_{2}^{-}, \mathrm{NO}_{3}^{-}\) c. \(\mathrm{OCl}^{-}, \mathrm{OI}^{-}\)

Classify each of the following as a strong acid, weak acid, strong base, or weak base in aqueous solution. a. \(\mathrm{HNO}_{2}\) b. \(\mathrm{HNO}_{3}\) c. \(\mathrm{CH}_{3} \mathrm{NH}_{2}\) d. \(\mathrm{NaOH}\) e. \(\mathrm{NH}_{3}\) f. \(\mathrm{HF}\) g. h. \(\mathrm{Ca}(\mathrm{OH})_{2}\) i. \(\mathrm{H}_{2} \mathrm{SO}_{4}\)
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