17.54 (a) The molar solubility of PbBr2 at 25 °C is 1.0 × 10-2 mol/L. Calculate Kp- (b) If 0.0490 g of AgIO3 dis- sp• solves per liter of solution, calculate the solubility-product constant. (c) Using the appropriate Ksp value from Appen- dix D, calculate the pH of a saturated solution of Ca(OH)2.
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17.54
Ksp= 6.5 x 10 -6
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- A buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M nitrous acid, HNO2. Assume no volume change after HNO2 is dissolved. Calculate the pH of this buffer.Marble is almost pure CaCO3. Acid rain has a devastating effect on marble statuary left outdoors. Assume that the reaction which occurs is CoCO3(s)+ H+(aq)Ca2+(aq)+HCO3(aq) Neglecting all other competing equilibria and using Tables 15.1 and 13.2, calculate (a) K for the reaction. (b) the molar solubility of CaCO3 in pure water. (c) the molar solubility of CaCO3 in acid rainwater with a pH of 4.00.A 250-mL buffer solution contains 0.0510 mole of KH2PO4 and 0.0875 mole of K2HPO4. (a) Calculate the molar concentrations of H2PO4–and HPO42–, respectively, in thesolution. (b) What is the pH of the solution? (H2PO4– has Ka = 6.2 x 10–8) (c) Write a net ionic equation for the buffering reaction against a strong acid by this buffer. (d) If 0.012 mole of hydrochloric acid (HCl) is added to the solution, create a reaction table to show the buffering reaction and calculate the molar concentration of H2PO4–and HPO42–, respectively, in the resulting solution after the buffering reaction. (e) What is the pH of the resulting solution?
- Your answer is partially correct. Ammonia is a convenient buffer system in the slightly basic range. (a) What is the pH of a buffer solution containing 46 g of NH4CI dissolved in 1.00 L of 0.920 M NH3? pH = 9.24 (b) How many moles of acid are required to change the pH of this solution by 0.07 pH units? i 5.5E-2 mol (c) Suppose 4.8 mL of 11.8 M HCI solution is added to 146 mL of the solution of Part (a). Calculate the new pH. pH = i 9.08 eTextbook and Media Save for Later Attempts: 1 of 3 used Submit AnswerA buffer contains 0.10 mol of acetic acid and 0.13 mol ofsodium acetate in 1.00 L. (a) What is the pH of this buffer?(b) What is the pH of the buffer after the addition of 0.02mol of KOH? (c) What is the pH of the buffer after the additionof 0.02 mol of HNO3?16.66 The molar solubility of AgCl in 6.5 x 10³M AGNO3 is 2.5 x 10-8 M. In deriving Kp from these data, which of the following assumptions are reasonable? (a) Ksp is the same as solubility. (b) Kp of AgCl is the same in 6.5 x 10 M AGNO3 as in pure water. ds. (c) Solubility of AgCl is independent of the concentration of AGNO3. (d) [Ag*] in solution does not change significantly upon the addition of AgCl to 6.5 × 10¬3 M AGNO3. (e) [Ag*] in solution after the addition of AgCl to 6.5 x 10 M AGNO3 is the same as it would be in pure water.
- A buffer solution contains 0.89 mol of phenol (HC6H5O) and 0.86 mol of sodium phenoxide (NaC6H5O) in 8.80 L.The Ka of phenol (HC6H5O) is Ka = 1.3e-10.(a) What is the pH of this buffer?pH = (b) What is the pH of the buffer after the addition of 0.25 mol of NaOH? (assume no volume change)pH = (c) What is the pH of the original buffer after the addition of 0.37 mol of HI? (assume no volume change)pH =A buffer solution contains 0.50 mol of hydrazoic acid (HN3) and 0.62 mol of sodium hydrazoate (NaN3) in 7.00 L. The K, of hydrazoic acid (HN3) is Ka = 1.9e-05.. (a) What is the pH of this buffer? pH = 5.96 (b) What is the pH of the buffer after the addition of 0.35 mol of NaOH? (assume no volume change) pH = 5.86 x pH = X (c) What is the pH of the original buffer after the addition of 0.35 mol of HI? (assume no volume change) xA buffer contains 0.15 mol of propionic acid (C2H5COOH)and 0.10 mol of sodium propionate (C2H5COONa) in 1.20 L.(a) What is the pH of this buffer? (b) What is the pH of thebuffer after the addition of 0.01 mol of NaOH? (c) What isthe pH of the buffer after the addition of 0.01 mol of HI?
- A chemistry graduate student is given 125. mL of a 1.50M diethylamine ((C,H, NH solution. Diethylamine is a weak base with K,=1.3 × 10 °. What mass (HIN %3D of (C,H5), NH,Br should the student dissolve in the (C,H,) NH solution to turn it into a buffer with pH =10.79? 2. You may assume that the volume of the solution doesn't change when the (C,H) NH, Br is dissolved in it. Be sure your answer has a unit symbol, and round 12 it to 2 significant digits. 10A buffer solution contains 0.40 mol of arsenous acid (H3AsO3) and 0.87 mol of sodium dihydrogen arsenite (NaH2AsO3) in 7.30 L.The Ka of arsenous acid (H3AsO3) is Ka = 5.1e-10. (a) What is the pH of this buffer?pH = (b) What is the pH of the buffer after the addition of 0.35 mol of NaOH? (assume no volume change)pH =A buffer solution contains 0.40 mol of arsenous acid (H3AsO3) and 0.87 mol of sodium dihydrogen arsenite (NaH2AsO3) in 7.30 L.The Ka of arsenous acid (H3AsO3) is Ka = 5.1e-10.(a) What is the pH of this buffer?pH = (b) What is the pH of the buffer after the addition of 0.35 mol of NaOH? (assume no volume change)pH = (c) What is the pH of the original buffer after the addition of 0.44 mol of HI? (assume no volume change)pH =