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Which is the stronger conjugate base, CN-or OCN-? Explain What is the K, for OCN-? [numerical...
please explain 3,4,and 5 thanks Diassociate 3. Which of the following is not a conjugate acid-base...
please explain 3,4,and 5
thanks
Diassociate 3. Which of the following is not a conjugate acid-base pair? a. H2SO4, SO4 b. HNO3, NO3 c. HC2H302, C2H302 d. H2PO4 , HPO4 e. HBr, Br 4. Which of the following is a conjugate acid-base pair? a. HNO3, H2NO3 b. HNH, NH, c. H F, HF d. HPO,2,PO e. HCN, CN 5. Choose the case that is not a Bronsted conjugate acid-base pair. a. CH3NH3", CH3NH2 b. HCN, CN c. HCIO, CIO2 d....
2. write the equation representing the weak base of the NH/NH.Chuffer in equilibrium with its conjugate...
2. write the equation representing the weak base of the NH/NH.Chuffer in equilibrium with its conjugate acid 3. Write the acid-dissociation-constant, ka, for the reaction in question 12. 4. Solve for the above equation for the [H+). 5. Write the chemical equation for the reaction that occurs when HNO, solution is added to the N solution. In other words, show which species in the buffer the acid would react with 6. What happens to the [NH) and (NH4"] when HNO,...
A buffer is composed of formic acid and its conjugate base, the formate ion. K, for...
A buffer is composed of formic acid and its conjugate base, the formate ion. K, for formic acid is 1.8 x 10- a What is the pH of a solution that has a formic acid concentration of 0.020 M and a sodium formate concentration of 0.055 M? pH = 4.18 Correct pK, = - log(1.8 x 10^4) = 3.74 We use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution. (HCO3 pH=pk.vlog HCO, = 3.74 +log 0.055 020...
please help me to break this into steps so that I can understand. thank you :) CNN CN + NH, Acid Base Base Acid 12....
please help me to break this into steps so that I can
understand. thank you :)
CNN CN + NH, Acid Base Base Acid 12. (6 points) Complete the following table. PH [H] (M) 0.0.0 10 Acidic / basic ! Q3 0 000 Acid 104 Base neutral Acid 13. (4 points) A buffer consists of HCO, and CO 2 a) Write the equation for the reaction when a strong acid (H,0") is added to the buffer #0 - co teo+HOU...
11. Which Brønsted-Lowry base has the strongest conjugate acid? A) CH.COM B) CN- C) F- D)...
11. Which Brønsted-Lowry base has the strongest conjugate acid? A) CH.COM B) CN- C) F- D) NOZ E) CIO 12. Which Brønsted-Lowry acid has the strongest conjugate base? A) HBr B) HCIOC) HFD) HI E) HNO3 13. Calculate the H30+ concentration in an aqueous solution that contains 2.50 x 104 M in OH-. A) 4.00 x 10-'M B) 4.00 10-10M C) 4.00 10-11 M. D) 5.00 10-11 M E) None of these 14) What is the pH of a 0.020...
CHE 172 Acid-Base Equilibrium Worksheet 1. Identify the conjugate pairs in the following reaction: HC2H302(aq) +...
CHE 172 Acid-Base Equilibrium Worksheet 1. Identify the conjugate pairs in the following reaction: HC2H302(aq) + H2O + H20*24) + CH3O2 (aq) 2. Based on the Kb of the following weak bases, which is the strongest base? C6H5NH2 HONH2 H2NNH2 C2H5NH2 Kb = 4.3x10-10 Ko = 1.1x10-8 Kb = 1.3x106 Kb = 6.4x104 Which has the strongest conjugate acid? 3. Calculate the pH of the following solutions: a. 0.25M HBO b. 0.25M Ba(OH)2 C. 0.25M HCN (K. = 5.00x10-10) d....
1. A hydrogen atom in the organic base pyridine, CsHsN, can be substituted by various atoms...
1. A hydrogen atom in the organic base pyridine, CsHsN, can be substituted by various atoms or groups to give XCsH4N, where X is an atom such as Cl or a group such as CH3. The following table gives K, values for the conjugate acids of a variety of substituted pyridines. Atom or Group X (aq) + HCl(aq) → (aq) + Cl-(aq) NO K, of Conjugate Acid 5.9 x 10-2 1.5 x 10-4 6.8 x 10-6 1.0 x 10-6 н....
++ ++ ++ ++ ++ If the Kh of a weak base is 7.7 x 10-6, what is the pH of a 0.48 M solution of this base? pH = Enough o...
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If the Kh of a weak base is 7.7 x 10-6, what is the pH of a 0.48 M solution of this base? pH = Enough of a monoprotic weak acid is dissolved in water to produce a 0.0136 M solution. The pH of the resulting solution is 2.42. Calculate the K, for the acid. Kg =
a. Write the net ionic equation for the acid-base hydrolysis equilibrium that is established when ammonium...
a. Write the net ionic equation for the acid-base hydrolysis equilibrium that is established when ammonium nitrate is dissolved in water.(Use H3O+ instead of H+.) Is the solution acidic/basic/neutral? b. Write the net ionic equation for the acid-base hydrolysis equilibrium that is established when ammonium chloride is dissolved in water. Is the solution acidic/basic/neutral?
Experiment 11-Pre-lab Questions listed give the conjugate base, and indicate if a solution of the conjugate...
Experiment 11-Pre-lab Questions listed give the conjugate base, and indicate if a solution of the conjugate acid-base pair would act as a buffer. Acid a. HCI b. HF e. HNO, d. CH,CO,H e. HBr Conjugate base CI- Buffered Solution? No 2. A buffered solution will resist changes in pH when small amounts of acid or base are added. However if a large amount of acid or base is added, the buffer will cease to work and a large pH change...
please explain 3,4,and 5
thanks
Diassociate 3. Which of the following is not a conjugate acid-base pair? a. H2SO4, SO4 b. HNO3, NO3 c. HC2H302, C2H302 d. H2PO4 , HPO4 e. HBr, Br 4. Which of the following is a conjugate acid-base pair? a. HNO3, H2NO3 b. HNH, NH, c. H F, HF d. HPO,2,PO e. HCN, CN 5. Choose the case that is not a Bronsted conjugate acid-base pair. a. CH3NH3", CH3NH2 b. HCN, CN c. HCIO, CIO2 d....
2. write the equation representing the weak base of the NH/NH.Chuffer in equilibrium with its conjugate acid 3. Write the acid-dissociation-constant, ka, for the reaction in question 12. 4. Solve for the above equation for the [H+). 5. Write the chemical equation for the reaction that occurs when HNO, solution is added to the N solution. In other words, show which species in the buffer the acid would react with 6. What happens to the [NH) and (NH4"] when HNO,...
A buffer is composed of formic acid and its conjugate base, the formate ion. K, for formic acid is 1.8 x 10- a What is the pH of a solution that has a formic acid concentration of 0.020 M and a sodium formate concentration of 0.055 M? pH = 4.18 Correct pK, = - log(1.8 x 10^4) = 3.74 We use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution. (HCO3 pH=pk.vlog HCO, = 3.74 +log 0.055 020...
please help me to break this into steps so that I can
understand. thank you :)
CNN CN + NH, Acid Base Base Acid 12. (6 points) Complete the following table. PH [H] (M) 0.0.0 10 Acidic / basic ! Q3 0 000 Acid 104 Base neutral Acid 13. (4 points) A buffer consists of HCO, and CO 2 a) Write the equation for the reaction when a strong acid (H,0") is added to the buffer #0 - co teo+HOU...
11. Which Brønsted-Lowry base has the strongest conjugate acid? A) CH.COM B) CN- C) F- D) NOZ E) CIO 12. Which Brønsted-Lowry acid has the strongest conjugate base? A) HBr B) HCIOC) HFD) HI E) HNO3 13. Calculate the H30+ concentration in an aqueous solution that contains 2.50 x 104 M in OH-. A) 4.00 x 10-'M B) 4.00 10-10M C) 4.00 10-11 M. D) 5.00 10-11 M E) None of these 14) What is the pH of a 0.020...
CHE 172 Acid-Base Equilibrium Worksheet 1. Identify the conjugate pairs in the following reaction: HC2H302(aq) + H2O + H20*24) + CH3O2 (aq) 2. Based on the Kb of the following weak bases, which is the strongest base? C6H5NH2 HONH2 H2NNH2 C2H5NH2 Kb = 4.3x10-10 Ko = 1.1x10-8 Kb = 1.3x106 Kb = 6.4x104 Which has the strongest conjugate acid? 3. Calculate the pH of the following solutions: a. 0.25M HBO b. 0.25M Ba(OH)2 C. 0.25M HCN (K. = 5.00x10-10) d....
1. A hydrogen atom in the organic base pyridine, CsHsN, can be substituted by various atoms or groups to give XCsH4N, where X is an atom such as Cl or a group such as CH3. The following table gives K, values for the conjugate acids of a variety of substituted pyridines. Atom or Group X (aq) + HCl(aq) → (aq) + Cl-(aq) NO K, of Conjugate Acid 5.9 x 10-2 1.5 x 10-4 6.8 x 10-6 1.0 x 10-6 н....
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If the Kh of a weak base is 7.7 x 10-6, what is the pH of a 0.48 M solution of this base? pH = Enough of a monoprotic weak acid is dissolved in water to produce a 0.0136 M solution. The pH of the resulting solution is 2.42. Calculate the K, for the acid. Kg =
Experiment 11-Pre-lab Questions listed give the conjugate base, and indicate if a solution of the conjugate acid-base pair would act as a buffer. Acid a. HCI b. HF e. HNO, d. CH,CO,H e. HBr Conjugate base CI- Buffered Solution? No 2. A buffered solution will resist changes in pH when small amounts of acid or base are added. However if a large amount of acid or base is added, the buffer will cease to work and a large pH change...
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