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HCN (aq) + HCO3(aq) → CN- (aq) + H₂CO3(aq) If K <1,what is the (a) strongest acid and the strongest base 2A Which of the species in # 1 can act as both a Bronsted acid and a Bronsted base

HCN (aq) + HCO3(aq) → CN- (aq) + H₂CO3(aq) If K <1,what is the (a) strongest acid and the strongest base 2A Which of the species in # 1 can act as both a Bronsted acid and a Bronsted base

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Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Answer 1A and 2A please. Show work and reasoning/explanation behind the answers. Clear typed answers, please Thank you
Chapter - 4A Given: HCN (aq) + HCO 3 (aq) → CN- (aq) + H₂CO3 (aq) If K <1, what is the (a) strongest acid and the strongest base 2A Which of the species in # 1 can act as both a Bronsted acid and a Bronsted base ? BA solution of 8.0 M formic acid (HCOOH) is 0.47 % ionized. What is the pH of the solution and Ka of HCOOH ? What is the pH of 0.10 M sodium carbonate solution ?Ka1 = 4.3 x 107 and Ka2= 5.6x10-¹¹ for H₂CO3(aq) What is the pH of a solution prepared by mixing 50.0 mL of a 0.10M solution of HF with 25.0 mL of a 0.20M solution of NaF? pka of HF = 3.14 € What is the pH of the solution prepared by adding 5.00 mL of 0.10M NaOH to solution in #5? F How much solid NaCN must be added to 1.0 L of a 0.50M HCN solution to give a pH of 7.00 ? Ka HCN= 6.2 x 10-10. We add some ammonium sulfate to water .What is the nature of the solution ,neutral, acidic, or basic. Write the hydrolysis equations and using Ka (NH4* )= 5.6x10-10 and Kb (SO42) -8.3x10-¹3 Explain your reasoning. H. 0.0100 mole of a weak acid (HA) was dissolved in water to make a 100.0 mL solution. A titration was performed using 0.100 M NaOH.After 40.00 mL of base was added the pH was 4.00. What is the Ka of the acid HA? Calculate the pH at the equivalence point when 0.104 g sodium acetate (MM-82.0,Kb-5.6x10-10) Is dissolved in water to make 25.0 mL of solution and titrated with 0.0996M HCL (aq) A solution is 0.10M in FeCl₂. What is the pH necessary to just prevent the formation of iron (II) sulfide when the solution is saturated with H₂S ? Ka1, H₂S= 1.00 x107,Ka2, HS-= 1.3 x10-13; Ksp FeS=4.9x10-18
Transcribed Image Text:Chapter - 4A Given: HCN (aq) + HCO 3 (aq) → CN- (aq) + H₂CO3 (aq) If K <1, what is the (a) strongest acid and the strongest base 2A Which of the species in # 1 can act as both a Bronsted acid and a Bronsted base ? BA solution of 8.0 M formic acid (HCOOH) is 0.47 % ionized. What is the pH of the solution and Ka of HCOOH ? What is the pH of 0.10 M sodium carbonate solution ?Ka1 = 4.3 x 107 and Ka2= 5.6x10-¹¹ for H₂CO3(aq) What is the pH of a solution prepared by mixing 50.0 mL of a 0.10M solution of HF with 25.0 mL of a 0.20M solution of NaF? pka of HF = 3.14 € What is the pH of the solution prepared by adding 5.00 mL of 0.10M NaOH to solution in #5? F How much solid NaCN must be added to 1.0 L of a 0.50M HCN solution to give a pH of 7.00 ? Ka HCN= 6.2 x 10-10. We add some ammonium sulfate to water .What is the nature of the solution ,neutral, acidic, or basic. Write the hydrolysis equations and using Ka (NH4* )= 5.6x10-10 and Kb (SO42) -8.3x10-¹3 Explain your reasoning. H. 0.0100 mole of a weak acid (HA) was dissolved in water to make a 100.0 mL solution. A titration was performed using 0.100 M NaOH.After 40.00 mL of base was added the pH was 4.00. What is the Ka of the acid HA? Calculate the pH at the equivalence point when 0.104 g sodium acetate (MM-82.0,Kb-5.6x10-10) Is dissolved in water to make 25.0 mL of solution and titrated with 0.0996M HCL (aq) A solution is 0.10M in FeCl₂. What is the pH necessary to just prevent the formation of iron (II) sulfide when the solution is saturated with H₂S ? Ka1, H₂S= 1.00 x107,Ka2, HS-= 1.3 x10-13; Ksp FeS=4.9x10-18
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