Homework Answers
a) The purpose of buffer is to maintain the pH
option 3
b) The salt of weak acid is needed to provide the conjugate base [ as its presence suppresses the dissociation of weak acid , thus provide resistance to pH change] which reacts with the added H3O+
option 1 and option 2 both.
c)
When OH- (base ) is added it is neutralized by the weak undissociated acid HF ( not by H3O+)
No correct option given.
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Consider the buffer system of hydrofluoric acid. HF. and its salt. NaF. HF(aq) + H2O() E H 0*(aq) + F(aq) a. The pu...
Question 1 1 pts Consider a solution that is 0.1 M HF and 0.1 M NaF....
Question 1 1 pts Consider a solution that is 0.1 M HF and 0.1 M NaF. This is a mixture of conjugates in equal proportions, which tells you that it is a buffer. What two reactions are relevant to the pH in this situation? NaF --> Nat + F F+H2O <--> HF + OH- HF + NaF --> H+ +Na+ + F2 HF <--> H+ +F Ht+F<--> Nat + F" Question 2 1 pts A buffer solution contains a mixture...
QUESTION 3 Which of the following statements is true regarding a buffer system of HF acid...
QUESTION 3 Which of the following statements is true regarding a buffer system of HF acid and its salt, NaF? The HF neutralizes the added acid. The HF neutralizes the added base. The NaF neutralizes the added H20. The HF is not a necessary component.
question 6 a-f 6. The dissociation reaction for hydrofluoric acid is shown below. HF (aq) =...
question 6 a-f
6. The dissociation reaction for hydrofluoric acid is shown below. HF (aq) = H (aq) + F (aq) a. Write an equilibrium expression for the dissociation reaction shown above. b. An HF solution at equilibrium is found to contain 0.0445 M HF, 0.00549 MH', and 0.00549 MF. Based on this information, what is the value of Key for the dissociation of HF? Show calculations to support your answer. A small amount of CaCl2 is added to the...
is a solution that resists changes in pH when a small amount of acid or base...
is a solution that resists changes in pH when a small amount of acid or base is added to best buffer solutions are prepared from weak acids and their conjugate base added as a sodium of potassium salt. Most biological systems must maintain a very narrow range of pH; therefore, buffers allow the biological solution to function correctly. Blood is a good example of a biological system that must maintain a pH in a very narrow range from 7.3 to...
Lab 8: Acids and Bases: Fill in these tables Acid Base Conjugate Acid HNO2 H2O HF...
Lab 8: Acids and Bases: Fill in these tables Acid Base Conjugate Acid HNO2 H2O HF H₂O HO" Conjugate Base Balanced Reaction HNO3 + H2O → NO,' + H2O F NH3 + HCN » NH+ CNC HCI NaOH H, O CIO, Which of the above could you make a buffer with? (using the Kor Na salt of the conjugate base of course) | (ОН) pH [H30] 2.5 x 100M Acidic, Basic or Neutral? 3.6 x 10M
1. A buffer is 0.100 M in HF and 0.100 M in NaF. When a small...
1. A buffer is 0.100 M in HF and 0.100 M in NaF. When a small
amount of nitric acid is added the pH only slightly drops. Write
the chemical equation that shows the added nitric acid being
neutralized by this buffer.
2. What is the pH of a buffer that is 0.120 M formic acid
(HCHO2) and 0.080 M in potassium formate (KCHO2)? The Ka of formic
acid is 1.8 x 10^ -4 .
3. The curve shows the...
HF(aq) + H2O() H0"(aq) + F (aq) EC. 2 H2O() H3O* (aq) + OH(aq) if [HFJinitial 0.05M, then K,=[H,O" ][A]/[HA...
HF(aq) + H2O() H0"(aq) + F (aq) EC. 2 H2O() H3O* (aq) + OH(aq) if [HFJinitial 0.05M, then K,=[H,O" ][A]/[HA] Kw=[HO"][OH] 0.05M [HF] +[F] equilibria (1) (2) mass balance (3) charge balance al+LHol L0H] (4) Given the setup above, manipulate the equations so you are left with this equation: Ka [H3O'1{[H,o'j-K[H3O']} / {0.05-[H20*1-K.//H2O]} ( you do not have to distribute the negative in the denominator)
HF(aq) + H2O() H0"(aq) + F (aq) EC. 2 H2O() H3O* (aq) + OH(aq) if...
HF(aq) + H2O() H0"(aq) + F (aq) EC. 2 H2O() H3O* (aq) + OH(aq) if [HFJinitial 0.05M, then K,=[H,O" ][A]/[HA...
HF(aq) + H2O() H0"(aq) + F (aq) EC. 2 H2O() H3O* (aq) + OH(aq) if [HFJinitial 0.05M, then K,=[H,O" ][A]/[HA] Kw=[HO"][OH] 0.05M [HF] +[F] equilibria (1) (2) mass balance (3) charge balance al+LHol L0H] (4) Given the setup above, manipulate the equations so you are left with this equation: Ka [H3O'1{[H,o'j-K[H3O']} / {0.05-[H20*1-K.//H2O]} ( you do not have to distribute the negative in the denominator)
HF(aq) + H2O() H0"(aq) + F (aq) EC. 2 H2O() H3O* (aq) + OH(aq) if...
A buffer solution is able to maintain a constant pH when small amounts of acid or...
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 mL solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O,. The initial concentration of both the acid and the base are 0.0100 mol/ 0.1000 L...
To understand how buffers use reserves of conjugate acid and conjugate base to counteract the effects...
To understand how buffers use reserves of conjugate acid and conjugate base to counteract the effects of acid or base addition on pH. A buffer is a mixture of a conjugate acid-base pair. In other words, it is a solution that contains a weak acid and its conjugate base, or a weak base and its conjugate acid. For example, an acetic acid buffer consists of acetic acid, CH3COOH, and its conjugate base, the acetate ion CH3COO−. Because ions cannot simply...
Question 1 1 pts Consider a solution that is 0.1 M HF and 0.1 M NaF. This is a mixture of conjugates in equal proportions, which tells you that it is a buffer. What two reactions are relevant to the pH in this situation? NaF --> Nat + F F+H2O <--> HF + OH- HF + NaF --> H+ +Na+ + F2 HF <--> H+ +F Ht+F<--> Nat + F" Question 2 1 pts A buffer solution contains a mixture...
QUESTION 3 Which of the following statements is true regarding a buffer system of HF acid and its salt, NaF? The HF neutralizes the added acid. The HF neutralizes the added base. The NaF neutralizes the added H20. The HF is not a necessary component.
question 6 a-f
6. The dissociation reaction for hydrofluoric acid is shown below. HF (aq) = H (aq) + F (aq) a. Write an equilibrium expression for the dissociation reaction shown above. b. An HF solution at equilibrium is found to contain 0.0445 M HF, 0.00549 MH', and 0.00549 MF. Based on this information, what is the value of Key for the dissociation of HF? Show calculations to support your answer. A small amount of CaCl2 is added to the...
is a solution that resists changes in pH when a small amount of acid or base is added to best buffer solutions are prepared from weak acids and their conjugate base added as a sodium of potassium salt. Most biological systems must maintain a very narrow range of pH; therefore, buffers allow the biological solution to function correctly. Blood is a good example of a biological system that must maintain a pH in a very narrow range from 7.3 to...
Lab 8: Acids and Bases: Fill in these tables Acid Base Conjugate Acid HNO2 H2O HF H₂O HO" Conjugate Base Balanced Reaction HNO3 + H2O → NO,' + H2O F NH3 + HCN » NH+ CNC HCI NaOH H, O CIO, Which of the above could you make a buffer with? (using the Kor Na salt of the conjugate base of course) | (ОН) pH [H30] 2.5 x 100M Acidic, Basic or Neutral? 3.6 x 10M
1. A buffer is 0.100 M in HF and 0.100 M in NaF. When a small
amount of nitric acid is added the pH only slightly drops. Write
the chemical equation that shows the added nitric acid being
neutralized by this buffer.
2. What is the pH of a buffer that is 0.120 M formic acid
(HCHO2) and 0.080 M in potassium formate (KCHO2)? The Ka of formic
acid is 1.8 x 10^ -4 .
3. The curve shows the...
HF(aq) + H2O() H0"(aq) + F (aq) EC. 2 H2O() H3O* (aq) + OH(aq) if [HFJinitial 0.05M, then K,=[H,O" ][A]/[HA] Kw=[HO"][OH] 0.05M [HF] +[F] equilibria (1) (2) mass balance (3) charge balance al+LHol L0H] (4) Given the setup above, manipulate the equations so you are left with this equation: Ka [H3O'1{[H,o'j-K[H3O']} / {0.05-[H20*1-K.//H2O]} ( you do not have to distribute the negative in the denominator)
HF(aq) + H2O() H0"(aq) + F (aq) EC. 2 H2O() H3O* (aq) + OH(aq) if...
HF(aq) + H2O() H0"(aq) + F (aq) EC. 2 H2O() H3O* (aq) + OH(aq) if [HFJinitial 0.05M, then K,=[H,O" ][A]/[HA] Kw=[HO"][OH] 0.05M [HF] +[F] equilibria (1) (2) mass balance (3) charge balance al+LHol L0H] (4) Given the setup above, manipulate the equations so you are left with this equation: Ka [H3O'1{[H,o'j-K[H3O']} / {0.05-[H20*1-K.//H2O]} ( you do not have to distribute the negative in the denominator)
HF(aq) + H2O() H0"(aq) + F (aq) EC. 2 H2O() H3O* (aq) + OH(aq) if...
A buffer solution is able to maintain a constant pH when small amounts of acid or base are added to the buffer. Consider what happens when 1 mL of a 5 M solution is added or 0.005 mol of HCl are added to a 100.0 mL solution acetic acid buffer that contains 0.0100 mol of Acetic acid, HC,H,O,, and 0.0100 mol of sodium acetate, NaC,H,O,. The initial concentration of both the acid and the base are 0.0100 mol/ 0.1000 L...
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