Please complete the table RTSort-Buffer SolutionsBuffer capacities in drops of baseBeaker #1Beaker #2Beaker #3Beaker #4Beaker #5Beaker #6до ӨZThinkVantageInitial2.714.154.524.915.228.10(10 drops3.924.534.805.266.6712.39PrtScSerl k20 dropsPause4.454.885.776.1911.5112.67InportColer, Madeleinemadeleine.coler@smail.pencol.edu30 drops4.81DolotoChoose...0 drops (Unable to buffer)10 drops base20 drops baseBuffer capacity was not reachedChoose...Choose...9.289.6812.3812.79BaseBuffer capactityChoose...Choose...Choose..Choose...Choose...Choose...Choose...Choose...Homo4)T510i5:29 PM8/14/2023Ⓡ3Ⓡ@ⒸⒸ3

Buffer capacity refers to the amount of acid or base required to change the pH of a buffer by one…

Buffer capacities in drops of base Beaker #1 Beaker #2 Beaker #3 Beaker #4 Beaker #5 Beaker #6 Initial 2.71 4.15 4.52 4.91 5.22 8.10 10 drops 3.92 4.53 4.80 5.26 6.67 12.39 20 drops 4.45 4.88 5.77 6.19 11.51 12.67 30 drops 4.81 9.28 Choose... 0 drops (Unable to buffer) 10 drops base 20 drops base Buffer capacity was not reached Choose... Choose... 9.68 12.38 Base Buffer capactity 12.79 Choose... Choose... Choose. Choose... Choose. Choose... Choose.. Choose... Ⓡ3 Ⓒ3 Ⓒ Ⓒ3

Buffer capacities in drops of base Beaker #1 Beaker #2 Beaker #3 Beaker #4 Beaker #5 Beaker #6 Initial 2.71 4.15 4.52 4.91 5.22 8.10 10 drops 3.92 4.53 4.80 5.26 6.67 12.39 20 drops 4.45 4.88 5.77 6.19 11.51 12.67 30 drops 4.81 9.28 Choose... 0 drops (Unable to buffer) 10 drops base 20 drops base Buffer capacity was not reached Choose... Choose... 9.68 12.38 Base Buffer capactity 12.79 Choose... Choose... Choose. Choose... Choose. Choose... Choose.. Choose... Ⓡ3 Ⓒ3 Ⓒ Ⓒ3

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.55QE

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For each of the following pairs of solutions, select the solution for which solute solubility is greatest. a. Ammonia gas in water with P = 1 atm and T = 50C Ammonia gas in water with P = 1 atm and T = 90C b. Carbon dioxide gas in water with P = 2 atm and T = 50C Carbon dioxide gas in water with P = 1 atm and T = 50C c. Table salt in water with P = 1 atm and T = 60C Table salt in water with P = 1 atm and T = 50C d. Table sugar in water with P = 2 atm and T = 40C Table sugar in water with P = 1 atm and T = 70C
Use this information to calculate Ka, for Ag, CO3. The solubility of Ag,CO, in water at 25 °C is measured to be 0.035 sp. Round your answer to 2 significant digits.
› Calculate the value of the equilibrium constant, Kỵ, for the reaction Q(g) + X(g) — 2M(g) + N(g) given that Kc = M(g) — Z(g) 6R(g) 2 N(g) + 4 Z(g) 3 X(g) + 3 Q(g) = 9R(g) Kc1 = 3.48 Kc2 Kc3 = 0.587 = = 13.6
Lead hydroxide, Pb(0H)2(s) | Pb(0H)2(s)Pb+2(aq)+20H-(aq) | Ksp=1.4x10-20 H2O(aq)H*(aq)+OH-(aq) Pb(OH)2 Water Kw=1.00x10-14 Molar masses 241.21 Pb 207.20 OH- 17.01 If Pb+2(aq) is controlled by the solubility of Pb(OH)2, what Pb+2(aq) concentration is expected if pH=p0H=7.00? b. What pH would be required to lower Pb+2(aq) to 2.07 ppb? a.
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The following system is at equilibrium in a closed vessel: 4 HCl(aq) + MnO2(s) ⇆ MnCl2(aq) + 2 Cl2(g) + 2 H2O(l) Various stresses are applied to the system as illustrated in the chart. Drag the appropriate label from the list below that indicates how the system responds to each stress. Each label can be used more than once.
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Sodium carbonate is a reagent that may be used to standardize acids in the same way that you have used KHP in this experiment. In such a standardization it was found that a 0.498-g sample of sodium carbonate required 24.8 mLmL mL of a sulfuric acid solution to reach the end point for the reaction. Na2CO3(aq)+H2SO4(aq)→H2O(l)+CO2(g)+Na2SO4(aq)Na2CO3(aq)+H2SO4(aq)→H2O(l)+CO2(g)+Na2SO4(aq) What is the molarity of the H2SO4H2SO4?
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