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Chapter 14: Q2 CYL (page 765)

14.2 What is the hydronium ion concentration in an aqueous solution with a hydroxide ion concentration of 0.001 M at 25̊C?

Short Answer

Expert verified

Hydronium [H3 O+] = 1.0× 10-11M

Step by step solution

01

To find the solution of hydroxide ion concentration of 0.001 M at 25̊C  

\begin{gathered} \left[ {O{H^ - }} \right] &= 0.001M \hfill \\K\omega & = \left[ {{H^ + }} \right]\left[ {o{H^ - }} \right] = 1{0^{ - 14}} \hfill \\ \left[ {{H^ + }} \right] &= \frac{{1{0^{ - 14}}}}{{[0H]}} &= \frac{{1{0^{ - 14}}}}{{0.001}}& = 1{0^{ - 11}}\;m \hfill \\ \left[ {{H_3}{o^ + }} \right] &= \left[ {{H^ + }} \right] &= 1.0 \times 1{0^{ - 11}}\;m \hfill \\ hydronium ion \left[ {{H_3}{o^ + }} \right] &= 1.0 \times 1{0^{ - 11}}M \hfill \\ \end{gathered}

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Most popular questions from this chapter

Which of the following concentrations would be practically equal in a calculation of the equilibrium concentrations in a \(0.134 - M\) solution of \({H_2}C{O_3}\), a diprotic acid: \(\left( {{H_3}{O^ + }} \right),\left( {O{H^ - }} \right),\left( {{H_2}C{O_3}} \right),\left( {HCO_3^ - } \right)\left( {CO_3^{2 - }} \right)?\) No calculations are needed to answer this question.

What is the effect on the concentration of hydrofluoric acid, hydronium ion, and fluoride ion when the following are added to separate solutions of hydrofluoric acid?

\(\begin{aligned}{l}(a)HCl\\(b)KF\\(c)NaCl\\(d)KOH\\(e)HF\end{aligned}\)

The equation for the equilibrium is \[HF(aq) + {H_2}O(l) \rightleftharpoons {H_3}{O^ + }(aq) + {F^ - }(aq)\]

Is the self ionization of water endothermic or exothermic? The ionization constant for water \(\left( {{K_W}} \right)\)is 2.9* \({10^{ - 14}}\)at \({40^ \circ }{\rm{C}}\)and 9.3 x \({10^{ - 14}}\)at \({60^ \circ }{\rm{C}}\)

What will be the\(pH\)of a buffer solution prepared from\(0.20\;mol N{H_3}, 0.40\;mol N{H_4}N{O_3}\), and just enough water to give\(1.00\;L\)of solution?

Nicotine, \({C_{10}}{H_{14}}\;{N_2}\), is a base that will accept two protons \(\left( {{K_1} = 7 \times 1{0^{ - 7}},{K_2} = 1.4 \times 1{0^{ - 11}}} \right)\). What is the concentration of each species present in a \(0.050 - M\) solution of nicotine?
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