Question 1 1 pts Consider a solution that is 0.1 M HF and 0.1 M NaF....
1. Which of the following make a buffer solution? (circle all the correct answers) a. 0.1 M HCl and 0.1 M NaCl b. 0.1 M HF and 0.075 M KF C. 0.15 M Pentanoic acid and 0.15 M sodium pentanoate d. 0.1 M NaOH and 0.1 M HCI e. 0.1 M acetic acid and 0.00001 sodium acetate 2. Which of the following could make buffer systems when mixed together? (circle the correct answers) a. 0.10 M acetic acid and 0.05...
Consider the buffer system of hydrofluoric acid. HF. and its salt. NaF. HF(aq) + H2O() E H 0*(aq) + F(aq) a. The purpose of this buffer system is to: 1. maintain (HF] 2. maintain [F] 3 maintain pH b. The salt of the weak acid is needed to: (1) provide the conjugate base 2. neutralize added 1,0 3. provide the conjugate acid c. If OH is added, it is neutralized by: 1. the salt 2. HO 3. H,00
Buffer action 4 A buffer solution consisting of 0.05 mol/L acetic acid (CH3COOH) and 0.05 mol/L acetate (CH3COO-) has been used to buffer a 1 L solution at pH 4.7. A small amount of sodium hydroxide solution containing 0.0001 mol NaOH was added. Which of the following reactions best represents the buffer action? + Select one: O a. NaOH(aq) Na+(aq) + OH(aq) O b. CH3COOH(aq) + H2O(1) CH3COO(aq) H30*(aq) O c. CH3COO(aq) + H2O(0) CH3COOH(aq) OH(aq) O d. CH3COOH(aq) +...
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...
As hydrogen ions, H+ are added to an acidic buffer solution made of acetic acid ( CH3COOH ) and sodium acetate, what happens to [CH3COOH ] and [ CH3COO¯ ] (conjugate base)? A. Both [CH3COOH ] and [ CH3COO¯ ] increase B. Both [CH3COOH ] and [ CH3COO¯ ] decrease C. [CH3COOH ] increases but [ CH3COO¯ ] decreases D. [CH3COOH ] decreases but [ CH3COO¯ ] increases
1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of HCl is added (Ka HC2H3O2 = 1.75 x 10-5). Report your answer to the hundredths place. 2) Calculate the pH of the 1L buffer composed of 500 mL 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of NaOH is added (Ka HC2H3O2 = 1.75...
A buffer is prepared by dissolving HF and NaF in water. Which of the following is the net ionic equation describing how the buffer neutralizes an acid (H+) that is added to the buffer? a. H+ + OH-H20 b. H+ + NaF-Nat + HF c. H + HF-HF d. H* + H20-H30* e. H +F HF For the reaction: N2(g) + 3H2(g) 22 NH3(g) first calculate AGº using values from Table 6, and then calculate AG at 298 K when...
Question 9 1 pts A certain buffer is 0.5 M HF and 0.3 M NaF. Which solution has the same pH as this buffer? 0.05 M HF and 0.03 M NaF 0.005 M HF and 0.003 M NaF OOO 0.0005 M HF and 0.0003 M NaF All of them have the same pH Question 10 Which buffer has the largest buffer capacity? 0.5 M HF and 0.3 M NaF 0.05 M HF and 0.03 M NaF 0.005 M HF and...
Given the following information: hydrofluoric acid HF acetic acidCH3COOH HF is a stronger acid than CH3COOH (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.056 M aqueous hydrofluoric acid and sodium acetate are mixed. It is not necessary to include states such as (aq) or (s). (2) Which is the strongest base, F or CH3coo? (3) At equilibrium the 7 will be favored. reactants products
1. (2 pts) Write the formula for the conjugate acid of the following bases: a. NH3 b.CO - 2. (2 pts) Which substance could you add to each solution to make it a buffer solution? b. 0.050 M HF C. 0.050 M CH3COOH 3. (2 pts) Calculate the concentration of H30* and OH-in a 1.5 M HCl solution. + Page 1 of 2 129 words CTX English (United States) Focus 140% equilibrium constant (K) of the neutralization reaction using the...