PRINCIPLES+REACTIONS
8th Edition
ISBN: 9781337759632
Author: Masterton
Publisher: CENGAGE L
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Chapter 14, Problem 16QAP
An aqueous solution of 0.057 M weak acid, HX, has a pH of 4.65. What is the pH of the solution if 0.018 mol of KX is dissolved in one liter of the weak acid?
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An aqueous solution of 0.057 M weak acid, HX, has a pH of 4.65. What is the pH of the solution if 0.018 mol of KX is dissolved in one liter of the weak acid?
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Chapter 14 Solutions
PRINCIPLES+REACTIONS
Ch. 14 - Write a net ionic equation for the reaction...Ch. 14 - Write a net ionic equation for the reaction...Ch. 14 - Write a balanced net ionic equation for the...Ch. 14 - Write a balanced net ionic equation for the...Ch. 14 - Calculate K for the reactions in Question 1.Ch. 14 - Calculate K for the reactions in Question 2.Ch. 14 - Prob. 7QAPCh. 14 - Calculate K for the reactions in Question 4.Ch. 14 - Calculate [H+] and pH in a solution in which...Ch. 14 - Calculate [OH-] and pH in a solution in which the...
Ch. 14 - A buffer is prepared by dissolving 0.0250 mol of...Ch. 14 - A buffer is prepared by dissolving 0.062 mol of...Ch. 14 - A buffer solution is prepared by adding 15.00 g of...Ch. 14 - A buffer solution is prepared by adding 5.50 g of...Ch. 14 - A solution with a pH of 9.22 is prepared by adding...Ch. 14 - An aqueous solution of 0.057 M weak acid, HX, has...Ch. 14 - Which of the following would form a buffer if...Ch. 14 - Which of the following would form a buffer if...Ch. 14 - Calculate the pH of a solution prepared by mixing...Ch. 14 - Calculate the pH of a solution prepared by mixing...Ch. 14 - Calculate the pH of a solution prepared by mixing...Ch. 14 - Calculate the pH of a solution prepared by mixing...Ch. 14 - Consider the weak acids in Table 13.2. Which...Ch. 14 - Prob. 24QAPCh. 14 - A sodium hydrogen carbonate-sodium carbonate...Ch. 14 - You want to make a buffer with a pH of 10.00 from...Ch. 14 - Prob. 27QAPCh. 14 - The buffer capacity indicates how much OH- or H+...Ch. 14 - A buffer is made up of 0.300 L each of 0.500 M...Ch. 14 - A buffer is made up of 239 mL of 0.187 M potassium...Ch. 14 - Enough water is added to the buffer in Question 29...Ch. 14 - Enough water is added to the buffer in Question 30...Ch. 14 - A buffer is prepared in which the ratio [ H2PO4...Ch. 14 - A buffer is prepared using the butyric...Ch. 14 - Blood is buffered mainly by the HCO3 H2CO3 buffer...Ch. 14 - There is a buffer system in blood H2PO4 HPO42 that...Ch. 14 - Given three acid-base indicators—methyl orange...Ch. 14 - Given the acid-base indicators in Question 37,...Ch. 14 - Metacresol purple is an indicator that changes...Ch. 14 - Thymolphthalein is an indicator that changes from...Ch. 14 - When 25.00 mL of HNO3 are titrated with Sr(OH)2,...Ch. 14 - A solution of KOH has a pH of 13.29. It requires...Ch. 14 - A solution consisting of 25.00 g NH4Cl in 178 mL...Ch. 14 - A 50.0-mL sample of NaHSO3 is titrated with 22.94...Ch. 14 - A sample of 0.220 M triethylamine, (CH3CH2)3 N, is...Ch. 14 - A 35.00-mL sample of 0.487 M KBrO is titrated with...Ch. 14 - A 0.4000 M solution of nitric acid is used to...Ch. 14 - A 0.2481 M solution of KOH is used to titrate...Ch. 14 - Consider the titration of butyric acid (HBut) with...Ch. 14 - Morphine, C17H19O3N, is a weak base (K b =7.4107)....Ch. 14 - Consider a 10.0% (by mass) solution of...Ch. 14 - A solution is prepared by dissolving 0.350 g of...Ch. 14 - Prob. 53QAPCh. 14 - Ammonia gas is bubbled into 275 mL of water to...Ch. 14 - For an aqueous solution of acetic acid to be...Ch. 14 - Prob. 56QAPCh. 14 - Prob. 57QAPCh. 14 - Water is accidentally added to 350.00 mL of a...Ch. 14 - A solution of an unknown weak base...Ch. 14 - Consider an aqueous solution of HF. The molar heat...Ch. 14 - Each symbol in the box below represents a mole of...Ch. 14 - Use the same symbols as in Question 61 ( = anion,...Ch. 14 - The following is the titration curve for the...Ch. 14 - Prob. 64QAPCh. 14 - Follow the directions of Question 64. Consider two...Ch. 14 - Prob. 66QAPCh. 14 - Indicate whether each of the following statements...Ch. 14 - Prob. 68QAPCh. 14 - Consider the following titration curves. The...Ch. 14 - Consider the titration of HF (K a=6.7104) with...Ch. 14 - The species called glacial acetic acid is 98%...Ch. 14 - Four grams of a monoprotic weak acid are dissolved...Ch. 14 - Prob. 73QAPCh. 14 - Fifty cm3 of 1.000 M nitrous acid is titrated with...Ch. 14 - A diprotic acid, H2B(MM=126g/moL), is determined...Ch. 14 - Prob. 76QAPCh. 14 - Two students were asked to determine the Kb of an...Ch. 14 - How many grams of NaOH must be added to 1.00 L of...Ch. 14 - How many grams of NaF must be added to 70.00 mL of...Ch. 14 - Prob. 80QAP
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- The Solubility Product Constant for manganese(II) carbonate is 1.8 × 10−¹¹ The molar solubility of manganese(II) carbonate in a water solution is M.arrow_forwardA buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500 mol·dm–3 HLac solution is mixed with 0.300 dm3 of the 0.300 mol·dm–3 NaLac solution to prepare the buffer. Ka for lactic acid (HLac) is 1.4 x 10-4 a) Calculate the pH of the lactic acid before it is mixed with the NaLac to form the buffer. b) Calculate the pH of the sodium lactate solution before it is mixed with the HLac to form the buffer. c) Calculate the pH of the buffer solution.arrow_forwardA titration involves adding a reactant of known quantity to a solution of an another reactant while monitoring the equilibrium concentrations. This allows one to determine the concentration of the second reactant. The equation for the reaction of a generic weak acid HA with a strong base is HA(aq) + OH(aq) →A¯(aq) + H₂O (1) A certain weak acid, HA, with a K, value of 5.61 x 10 ", is titrated with NaOH. 6 Part A A solution is made by titrating 9.00 mmol (millimoles) of HA and 2.00 mmol of the strong base. What is the resulting pH? Express the pH numerically to two decimal places. ▸ View Available Hint(s) pH = Submit ▾ Part B pH = IVE] ΑΣΦ Submit A → c More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 66.0 mL ? Express the pH numerically to two decimal places. ▸ View Available Hint(s) IVE ΑΣΦ A + Ċ ? Doowoon Review | Constants | Periodic Table ?arrow_forward
- A chemistry graduate student is given 250. mL of a 1.50M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K,=4.9 × 10 1º. What mass of NaCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 8.84? You may assume that the volume of the solution doesn't change when the NaCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ?arrow_forwardA 10.0 mL sample of 0.20 mol/L NiF2(aq) is mixed with 20.0 mL of 0.0700 mol/L NaOH(aq) and then diluted to a final volume of 100. mL. Calculate the concentration of OH- ions in the 100 mL mixture before the reaction starts. Express your answer to three significant figures.arrow_forwardAn aqueous solution of 0.1 M H2SO4(aq) is added to 0.1 M Na2S(aq) and is allowed to react. From the following, select all of the statements that are true. The product of the reaction will have a colored supernatant The product of the reaction will have a colorless supernatant The reaction will produce water as a product The reaction will produce a precipitate The reaction will produce a gas The reaction will result in an oxidation and/or reduction of one of the reactantsarrow_forward
- A chemist is performing a titration in order to determine the amount of sodium hydroxide, NaOH(aq), in 125 mL of an aqueous solution. (a) If 28 mL of a 0.13 M HCl solution was used as a titrant to reach the equivalence point, what was the concentration of sodium hydroxide in the initial solution? M (b) What was the initial pH of the sodium hydroxide solution?arrow_forwardWhat volume of 0.250 M HCl(aq) will completely react with 50.0 mL of 0.115 M NaOH(aq)? Write the balanced reaction and show the stoichiometry. Write the reaction of acetate ion in water. Predict the approximate pH of a solution with acetate ion present.arrow_forwardCalcium oxalate is a sparingly soluble ionic compound composed of calcium ions (Ca2+) and oxalate ions (C2O42–). It is a main culprit in kidney stone disease due to the formation of calcium oxalate crystals in the urine. A typical value for the concentration of calcium in urine is 0.3 grams per liter. Given a Ksp value for calcium oxalate of 1.3 × 10–8, calculate the minimum concentration of oxalate ion in urine that could lead to precipitation of calcium oxalate.arrow_forward
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