11:39Buffer solution pH calculations | Chemistry | Khan AcademyKhan Academy Organic Chemistry665views
Multiple ChoiceWhich one of the following combinations does not create a buffer?1314views2rank11commentsHas a video solution.
Multiple ChoiceWhich of the following combinations can result in the formation of a buffer?1440views4rank7commentsHas a video solution.
Multiple Choice Which of the following combinations can result in the formation of a buffer?1419views1rank5commentsHas a video solution.
Multiple ChoiceA buffer solution is comprised of 50.0 mL of a 0.100 M HC2H3O2 and 60.0 mL of a 0.100 M NaC2H3O2. Which of the following actions would completely destroy the buffer?1898views3rank9commentsHas a video solution.
Multiple ChoiceCalculate the pH of a solution formed by mixing 200 mL of a 0.400 M C2H5NH2 solution with 350 mL of a 0.450 M C2H5NH3+ solution. (Kb of C2H5NH2 is 5.6 x 10 -4).2295views2rank19commentsHas a video solution.
Multiple ChoiceDetermine how many grams of sodium acetate, NaCH3CO2 (MW:82.05 g/mol), you would mix into enough 0.065 M acetic acid CH3CO2H (MW:60.05 g/mol) to prepare 3.2 L of a buffer with a pH of 4.58. The Ka is 1.8 x 10-5.2584views9commentsHas a video solution.
Multiple ChoiceA buffer solution is made by combining a weak acid with its conjugate salt. What will happen to the pH if the solution is diluted to one-fourth of its original concentration?1980views2commentsHas a video solution.
Multiple ChoiceWhich of the following statements is true about a solution prepared with equal amounts of HNO2 and NaNO2?206views
Multiple ChoiceThe addition of which of the following would destroy a 1.0 L buffer that is 0.50 M HC2H3O2 and 0.40 M NaC2H3O2?214views
Multiple ChoiceWhat is the pH of a 1.0 L buffer solution containing 0.500 M HF and 0.300 M NaF. Ka for HF = 3.5 × 10−4.314views
Multiple ChoiceDetermine the pH of a 1.0 L buffer prepared by adding 0.100 moles of NaOH to 0.250 moles of HF. Ka for HF = 3.5 × 10−4.208views
Multiple ChoiceWhat mass of NaC2H3O2 (molar mass = 82.03 g/mol) would need to be added to 0.450 moles of HC2H3O2 to prepare a 1.0 L buffer with a pH = 4.95. Ka for HC2H3O2 = 1.8 × 10−5.782views
Multiple Choice1.0 L of a buffer is prepared to produce a solution that is 0.400 M in HF and 0.250 M in LiF. What is the pH after the addition of 2.5 g of KOH? Assume no volume change. Ka for HF = 3.5 × 10−4.256views
Multiple ChoiceWhich pairs of compounds are capable of making a buffer? Select all that apply.a) 1.3 M LiOH and 1.7 M HCOOH c) 0.35 M CH3CO2H and 0.35 M NaOHb) 0.784 M NH4+ and 0.800 M HClO4 d) 0.80 HNO3 and 0.15 MgO235views5rankHas a video solution.
Multiple ChoiceDetermine which of the following actions will destroy a buffer composed of 0.50 L of 1.44 M H3PO4 and 0.60 L of 1.25 M NaH2PO4−.a) Addition of 1.45 moles of KH2PO4b) Addition of 0.85 moles of HClc) Addition of waterd) Addition of 0.30 moles of Ca(OH)2e) Addition of 0.70 moles of HIO4259views4rankHas a video solution.
Open QuestionA buffer resists change in ph when ___________ amount of acid or base is added to it.52viewsHas a video solution.
Textbook QuestionThe beaker on the right contains 0.1 M acetic acid solution with methyl orange as an indicator. The beaker on the left contains a mixture of 0.1 M acetic acid and 0.1 M sodium acetate with methyl orange. (b) Which solution is better able to maintain its pH when small amounts of NaOH are added? Explain. [Sections 17.1 and 17.2] 549viewsHas a video solution.
Textbook QuestionThe following diagram represents a buffer composed of equal concentrations of a weak acid, HA, and its conjugate base, A-. The heights of the columns are proportional to the concentrations of the components of the buffer. (c) Which of the three represents a situation that cannot arise from the addition of either an acid or a base? [Section 17.2] 607viewsHas a video solution.
Textbook QuestionThe following diagram represents a buffer composed of equal concentrations of a weak acid, HA, and its conjugate base, A-. The heights of the columns are proportional to the concentrations of the components of the buffer. (a) Which of the three drawings, (1), (2), or (3), represents the buffer after the addition of a strong acid? [Section 17.2] 314viewsHas a video solution.
Textbook QuestionWhat is the pH of a buffer solution prepared by dissolving 0.250 mol of NaH2PO4 and 0.075 mol of NaOH in enough water to make 1.00 L of solution? (Ka (H2PO4-) = 6.2 X 10^-8) (a) 6.32 (b) 6.83 (c) 7.21 (d) 7.71921viewsHas a video solution.
Textbook QuestionBars of iron are put into each of the three beakers as shown here. In which beaker—A, B, or C—would you expect the iron to show the most corrosion ? [Section 20.8] 461viewsHas a video solution.
Textbook QuestionA solution containing sulfide ions is added to a solution of 0.036 M Cu2+ and 0.044 M Fe2+. At what concentration of sulfide ion will a precipitate begin to form? What is the identity of the precipitate? (a) 1.4 x 10^-16 M, FeS (b) 3.6 x 10^-35 M, CuS (c) 3.6 x 10^-35 M, FeS (d) 1.4 x 10^-16 M, C280viewsHas a video solution.
Textbook QuestionWhich of the following solutions is a buffer? (a) A solution made by mixing 100 mL of 0.100 M CH3COOH and 50 mL of 0.100 M NaOH, (b) a solution made by mixing 100 mL of 0.100 M CH3COOH and 500 mL of 0.100 M NaOH, (c) A solution made by mixing 100 mL of 0.100 M CH3COOH and 50 mL of 0.100 M HCl, (d) A solution made by mixing 100 mL of 0.100 M CH3COOK and 50 mL of 0.100 M KCl.4080views1rankHas a video solution.
Textbook QuestionYou have to prepare a pH = 3.50 buffer, and you have the following 0.10 M solutions available: HCOOH, CH3COOH, H3PO4, HCOONa, CH3COONa, and NaH2PO4. Which solutions would you use?1726views1rankHas a video solution.
Textbook QuestionYou have to prepare a pH = 5.00 buffer, and you have the following 0.10 M solutions available: HCOOH, HCOONa, CH3COOH, CH3COONa, HCN, and NaCN. Which solutions would you use?675viewsHas a video solution.
Textbook QuestionA buffer contains significant amounts of acetic acid and sodium acetate. Write equations showing how this buffer neutralizes added acid and added base.2703viewsHas a video solution.
Textbook QuestionConsider the following table of standard reduction potentials: (b) Which substances can be oxidized by B2+? Which can be reduced by D?417viewsHas a video solution.
Textbook QuestionA buffer contains significant amounts of ammonia and ammonium chloride. Write equations showing how this buffer neutralizes added acid and added base.1597viewsHas a video solution.
Textbook QuestionThe following pictures represent solutions that contain one or more of the compounds H2A, NaHA, and Na2A, where H2A is a weak diprotic acid. (Na+ ions and solvent water molecules have been omitted for clarity.) (b) Which solution has the greatest buffer capacity?734viewsHas a video solution.
Textbook QuestionThe following pictures represent solutions that contain one or more of the compounds H2A, NaHA, and Na2A, where H2A is a weak diprotic acid. (Na+ ions and solvent water molecules have been omitted for clarity.) (a) Which of the solutions are buffer solutions?312viewsHas a video solution.
Textbook QuestionDetermine whether or not the mixing of each pair of solutions results in a buffer. e. 125.0 mL of 0.15 M NH3; 150.0 mL of 0.20 M NaOH450viewsHas a video solution.
Textbook QuestionDetermine whether or not the mixing of each pair of solutions results in a buffer. d. 175.0 mL of 0.10 M NH3; 150.0 mL of 0.12 M NaOH339viewsHas a video solution.
Textbook QuestionDetermine whether or not the mixing of each pair of solutions results in a buffer. c. 50.0 mL of 0.15 M HF; 20.0 mL of 0.15 M NaOH344viewsHas a video solution.
Textbook QuestionDetermine whether or not the mixing of each pair of solutions results in a buffer. b. 50.0 mL of 0.10 M HCl; 35.0 mL of 0.150 M NaOH418viewsHas a video solution.
Textbook QuestionDetermine whether or not the mixing of each pair of solutions results in a buffer. a. 100.0 mL of 0.10 M NH3; 100.0 mL of 0.15 M NH4Cl567viewsHas a video solution.
Textbook QuestionDetermine whether or not the mixing of each pair of solutions results in a buffer. e. 105.0 mL of 0.15 M CH3NH2; 95.0 mL of 0.10 M HCl677viewsHas a video solution.
Textbook QuestionDetermine whether or not the mixing of each pair of solutions results in a buffer. c. 165.0 mL of 0.10 M HF; 135.0 mL of 0.050 M KOH431viewsHas a video solution.
Textbook QuestionDetermine whether or not the mixing of each pair of solutions results in a buffer. b. 150.0 mL of 0.10 M HF; 135.0 mL of 0.175 M HCl2488views1rankHas a video solution.
Textbook QuestionThe fluids within cells are buffered by H2PO4- and HPO42 - . b. Could a buffer system employing H3PO4 as the weak acid and H2PO4- as the weak base be used as a buffer system within cells? Explain.1457views1rankHas a video solution.
Textbook QuestionA 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Determine if each addition would exceed the capacity of the buffer to neutralize it. d. 1.35 g HI807viewsHas a video solution.
Textbook QuestionA 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Determine if each addition would exceed the capacity of the buffer to neutralize it. b. 350 mg KOH1177viewsHas a video solution.
Textbook QuestionA 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Determine if each addition would exceed the capacity of the buffer to neutralize it. c. 1.25 g HBr800views1commentsHas a video solution.
Textbook QuestionA 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Determine if each addition would exceed the capacity of the buffer to neutralize it. a. 250 mg NaOH989viewsHas a video solution.
Textbook QuestionWhich of the following gives a buffer solution when equal volumes of the two solutions are mixed? (a) 0.10 M NH3 and 0.10 M HCl (b) 0.20 M NH3 and 0.10 M HCl (c) 0.10 M NH4Cl and 0.10 M NH3 (d) 0.20 M NH4Cl and 0.10 M NaOH3188viewsHas a video solution.
Textbook QuestionWhich of the following solutions has the greater buffer capacity: 100 mL of 0.30 M HNO2-0.30 M NaNO2 or 100 mL of 0.10 M HNO2-0.10 M NaNO2? Explain.1336viewsHas a video solution.
Textbook QuestionYou need a buffer solution that has pH = 7.00. Which of the following buffer systems should you choose? Explain. (a) H3PO4 and H2PO4 - (b) H2PO4- and HPO42- (c) HPO42- and PO43-1231viewsHas a video solution.
Textbook QuestionConsider a buffer solution that contains equal concentrations of H2PO4- and HPO42-. Will the pH increase, decrease, or remain the same when each of the following substances is added? (a) Na2HPO4 (b) HBr (c) KOH (d) KI (e) H3PO4 (f) Na3PO4878views1rankHas a video solution.
Textbook QuestionTwo buffers are prepared by adding an equal number of moles of formic acid (HCOOH) and sodium formate (HCOONa) to enough water to make 1.00 L of solution. Buffer A is prepared using 1.00 mol each of formic acid and sodium formate. Buffer B is prepared by using 0.010 mol of each. (b) Which buffer will have the greater buffer capacity?1415viewsHas a video solution.
Textbook QuestionConsider a galvanic cell that utilizes the following half-reactions: (d) Will AgCl precipitate if 10.0 mL of 0.200 M NaCl is added to the solution in part (c)? Will AgBr precipitate if 10.0 mL of 0.200 M KBr is added to the resulting solution?568viewsHas a video solution.
Open QuestionWhich of the following solutions represents a good buffer system?58viewsHas a video solution.
Open QuestionA solution that resists a change in ph when an acid or base is added to it is a(n) __________.57viewsHas a video solution.
Open QuestionSelect the statement that best describes a buffer. see concept 3.3 (page)59viewsHas a video solution.
Open QuestionA(n) is a substance or a mixture of substances that act to resist changes in pH.48viewsHas a video solution.
Open QuestionWhich of the following is a means of creating a buffer of H2CO3/NaHCO3₃?56viewsHas a video solution.
Open QuestionWhich of the following aqueous solutions are good buffer systems?57viewsHas a video solution.