Scholarship Ap X Report - Googl X NGLSync Portal X OWLv2 | Online X + entActivity.do?locator=assignment-take Use the References to access important values if needed for this question. The hydronium ion concentration of an aqueous solution of 0.422 M benzoic acid, C6H5COOH (Ka = 6.30x10-5) is [H3O+]= M. Submit Answer Retry Entire Group 9 more group attempts remaining 64°F ted 21 99+) a OF 40 9:47 PM 5/28/202

Scholarship Ap X Report - Googl X NGLSync Portal X OWLv2 | Online X + entActivity.do?locator=assignment-take Use the References to access important values if needed for this question. The hydronium ion concentration of an aqueous solution of 0.422 M benzoic acid, C6H5COOH (Ka = 6.30x10-5) is [H3O+]= M. Submit Answer Retry Entire Group 9 more group attempts remaining 64°F ted 21 99+) a OF 40 9:47 PM 5/28/202

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter16: Solubility And Complex Ion Equilibria

Section: Chapter Questions

Problem 10RQ: Figure 15-3 outlines the classic scheme for separating a mixture of insoluble chloride salts from...

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What fraction (percentage) ionizes in a 2.50 M C6H5OH (Ka = 1.0 x 10-10)?
Hello, can someone please help me with these chem questions and give me a clear step-by-step solution. Thank you very much for your help. a)The [H3O+], in M, of 10.00 mL of 0.100 M NaOH after adding 10.00 mL of indicator solution. To enter exponential values, use the format 1.0e-5. b)The [H3O+], in M, of 10.00 mL of 0.100 M HCl after adding 10.00 mL of the indicator solution. To enter exponential values, use the format 1.0e-5.
Figure 15-3 outlines the classic scheme for separating a mixture of insoluble chloride salts from one another. Explain the chemistry involved in the various steps of the figure.
6 What is the approximate freezing point of a 0.50 M solution of dichloroacetic acid, HC2HO2Cl2 (Ka=5.0 x 10-2)? Assuming the density of the solution is 1.0 g/mL. The freezing point depression constant for water equals –1.86 °C/m.
if all the N in 10.0 mmols urea, CO(NH2)2, is converted to NH4HSO4, and if, with excess NaOH, the NH3 is evolved and caught in 50.0 mL of HCl (1.00 mL = 0.03000 g CaCO3), what volume of NaOH (1.00 mL = 0.3465 g H2C2O4. H2O) would be required for complete titration? using Kjeldahl's Method
What is the Qsp of a solution mixture Al(OH)3 formed from 10 mL 1.00M C6H5NH2 and 15 mL 0.10M Al(NO3)3?
a) Calculate the pH of an aqueous solution of the salt NaA, which was made to a concentration of 0.080 M NaA. The Ka of the weak acid HA is 2.0 x 10-5. Your pH should go to two places past the decimal point (i.e. 1.35). b) Aniline, C6H5NH2, has a pKb of 9.40. What is the pH of a solution which is 0.12 M in aniline and 0.38 M in anilinium ion, C6H5NH3+? Your answer should be to two places past the decimal.
Why is H3O=[OH- ]=1.0 x 10-2 M not feasible in water? What would happen if we tried to make such a solution by mixing 1.0 x 10-2 molL of KOH with 1.0 x 10-2 molLHCl?
Construct a curve for the titration of 20.00 mL 0.500 N succinic acid (HO2CCH2CH2CO2H) by 0.1000 N NaOH solution. Use MS Excel for convenience. Titrant volumes: 0.00 mL, 5.00 mL, 10.00 mL, 15.00 mL, 20.00 mL, 25.00 mL, and 30.00 mL. (CH2)2(CO2H)2⇄(CH2)2(CO2H)(CO2)^- +H^+ Ka1= 6.21 x 10^-5; pKa1 =4.207 (CH2)2(CO2H)(CO2)^-⇄(CH2)2(CO2)2^2-+ H^+ Ka2= 2.31 x 10^-6; pKa2 =5.636
Explain why the pH of mixture C is the same as the pH of mixture A C) Mixture made by mixing equal volumes of 0.2 mol L–1 HCl and 0.2 mol L–1 NaCl Conductivity (mA) 340 PH 1 A 0.1 mol L–1 HCl 260 1
How to answer for Ka/ Kb and calculated pH of a solution? I think solution 1,2 only has one Ka/Kb value then the other Sol. 3,4. Then with calculated pH, pH = -log[H+] (acid) and pH = 14 + log[OH-] (base) is utilized. Though I do not know how getting the Ka/Kb will be used to get pH Ex. Solution 1: 30.0 mL 0.10 M CH3COOHSolution 2: 15.0 mL 0.20 M CH3COOH – 15.0 mL 0.20 M NaCH3COOSolution 3: 30.0 mL 0.10 M NH3Solution 4: 15.0 mL 0.20 M NH3 – 15.0 mL 0.20 M NH4Cl Sol 1,2 used methyl orange as indicatorSol 3,4 used phenolphthalein as indicator Solution w/ measured pH Ka/Kb Calculated pH 1 a 1.0 M HCl (2.01pH) b 1.0 M NaOH (3.98pH) c Control (2.91pH) 2 a 1.0 M HCl (4.73) b 1.0 M NaOH (4.82) c Control (4.76) 3. a 1.0 M HCl (10.09) b 1.0 M NaOH (11.98) c Control (11.11) 4. a 1.0 M HCl (9.13) b 1.0 M NaOH (9.38) c Control (9.30)
Bar Keepers Friend is a household cleaner containing oxalic acid, a diprotic acid where pKa1 = 1.27 and pKa2 = 4.27. If the molarity of oxalic acid in one bottle of Bar Keepers Friend is 0.458 M, explain how you would determine the fractional composition of the charge state [H2A] at pH = 3.98? Write out exactly how you would solve the problem (including plugging in the appropriate numerical values to solve the problem without actually calculating the final answer).