You have two aqueous solutions, (1) and (2), at 45°C. Fill in the missing values for each of these solutions in the table below. (At 45°C, the ion-product constant for water is 3.94x10-14, pK, = 13.405.) pH pOH [H,o+] (M) [OH-] (M) (1) 5.50 (2) 4.2x10-10 Step 1 of 10 Write the equation that defines pH in terms of the concentration of hydronium (or hydrogen) ions. The pH of a solution is given by the following equation. O pH = log[H,0*] O pH = In[H;0* ] O pH = -In[H,0* ] -log[H;0+ ] OpH = In this equation [H,0+] is the molar concentration of H,0+ ions. Step 2 of 10 Write the equation that defines pOH in terms of the concentration of hydroxide ions. The pOH of a solution is given by the following equation. O pOH = In[OH- ] O pOH = log[OH ] O pOH = -In[OH¯] PPOH = -log[OH-] In this equation [OH-] is the molar concentration of OH- ions. Step 3 of 10 Write the equation that defines the ion-product constant for water in terms of the concentrations of hydronium ions and hydroxide ions. The ion-product constant for water (K) is given by the following equation. (Equilibrium expressions take the general form: Ke = [C]° / [A]a . [B]b. Subscripts and superscripts that include letters must be enclosed in braces {}.) chemPad Help Greek -

2,4,7,8

Dissolved carbon dioxide in seawater occurs mainly in three inorganic forms (see figure below): free aqueous carbon dioxide (CO2(aq)), bicarbonate (HCO3), and carbonate ions (CO3²). (a) Using the figure, rank the concentrations of these species from highest to lowest. (b) If surface ocean pH were to fall from 8.0 to 7.0, how would this ranking change? -1.5 2 H+ Surface Ocean pH OH HCO3 -2.5 -3 CO₂ Log [concentration (mol kg¹)] сл + -4.5 50 2 4 6 PH 8 10 co 123 12 14

13. A 60.00 mL sample of 0.075 M sodium benzoate (NaC7H5O2) was titrated with 0.050 M HCl. What is the pH of the solutionafter 10.00 ml of HCl is added?(a) 4.19(b) 5.09(c) 5.74(d) 6.2414. What is the ratio of moles of benzoate (C7H5O2‒) to benzoic acid (HC7H5O2) in the solution that results from thecombination of the NaC7H5O2 and HCl in the problem above?(a) 8(b) 0.125(c) 0.0040(d) 0.00050

NH4+ (ap) + (1-(4) NH4C) (3) You are asked to bring the pH of 0.500 L of 0.500 mol/L NH4Cl to 7.00. What volume, in drops, (1 drop = 0.05 mL) of which of the following solutions would you use: 10.0 mol/L HCl or 10.0 mol/L NH3?

9. The base ionization constant K, describes which of the following reactions for a weak base, B, in aqueous solution? (а) в + н' BH B+ H,0° BH + H,0 (с) в -но ВН + ОН (d) в + он ВН + ОН (е) в -но BH + 0

Calculate [H], [CIO], and [OH-] in an aqueous solution that is 0.175 M in HClO4 (aq) at 25 °C. [H+] = x10 [CIO] = [OH-] = TOOLS y M M M

HCN has a K, of 4.9 X 10-10. What is the pH of a solution which contains 0.350 M NạCN? CN (aq) + H,O (1) HCN (aq) + Oн (аq)

Be sure to answer all parts. Calculate the hydroxide ion concentrations of the following solutions at 25°C, given the pOH. (a) pOH= 8.89 x 10 M |-[_HO] (Enter your answer in scientific notation.) (b) рОН - 4.52 M -[ HO] < Prev 15 of 28

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