To make 1.00 L of a 0.100 M H2PO4- / HPO42- buffer at pH 6.90 and you start with the NaH2PO4,
A. Calculate the mass of NaH2PO4 needed to make the buffer.
B. Should HCl or NaOH be added to make the final buffer? Calculate the number of moles of HCl or NaOH that needs to be added. Note: formula mass of NaH2PO4 is 120.
To make 1.00 L of a 0.100 M H2PO4- / HPO42- buffer at pH 6.90 and...
Part 1: Which pair of substances would make a good buffer system? a. H2PO4-/HPO42- b. H2PO4-/HPO42 c. SO42-/H2SO4 d. HCl/NaOH Part 2: Should the concentrations of the two buffer components be present at relatively high and concentrations close to each other or low with concentrations far from each other ? a. far and low b. close and high
You are instructed to create 400. mL of a 0.40 M phosphate buffer with a pH of 6.4. You have phosphoric acid and the sodium salts NaH2PO4, Na2HPO4, and Na3PO4 available. (Enter all numerical answers to three significant figures.) H3PO4(s) + H2O(l) H3O+(aq) + H2PO4−(aq) Ka1 = 6.9 ✕ 10−3 H2PO4−(aq) + H2O(l) H3O+(aq) + HPO42−(aq) Ka2 = 6.2 ✕ 10−8 HPO42−(aq) + H2O(l) H3O+(aq) + PO43−(aq) Ka3 = 4.8 ✕ 10−13 Which of the available chemicals will you use...
If you are to prepare a 1.000 L of a 0.100 M buffer at pH 5.00 using the CH3COOH/ Na+CH3COO- buffer system (pKa 4.76a), answer the following questions: What is the molar ratio of the base to acid at pH 5.0? The concentration of the buffer (0.100 M in this example) refers to the sum of the weak acid and its conjugate base. Given this information, what is the concentration of the weak acid and its conjugate base at pH...
You are instructed to create 200. mL of a 0.63 M phosphate buffer with a pH of 6.0. You have phosphoric acid and the sodium salts NaH2PO4, Na2HPO4, and Na3PO4 available. (Enter all numerical answers to three significant figures.) H3PO4(s) + H2O(l) equilibrium reaction arrow H3O+(aq) + H2PO4−(aq) Ka1 = 6.9 ✕ 10−3 H2PO4−(aq) + H2O(l) equilibrium reaction arrow H3O+(aq) + HPO42−(aq) Ka2 = 6.2 ✕ 10−8 HPO42−(aq) + H2O(l) equilibrium reaction arrow H3O+(aq) + PO43−(aq) Ka3 = 4.8 ✕ ...
You are instructed to create 400. mL of a 0.39 M phosphate buffer with a pH of 6.2. You have phosphoric acid and the sodium salts NaH2PO4, Na2HPO4, and Na3PO4 available. (Enter all numerical answers to three significant figures.) H3PO4(s) + H20(I) =H30+ (aq) + H2PO4 (aq) Kai = 6.9x10-3 H2PO4 (aq) + H20(1) =H30+ (aq) + HPO42-(aq) Ka2 = 6.2 x 10-8 HPO42-(aq) + H20(1) = H30+(aq) + PO43-(aq) Ka3 = 4.8x10-13 Which of the available chemicals will you...
You are instructed to create 400. mL of a 0.39 M phosphate buffer with a pH of 6.2. You have phosphoric acid and the sodium salts NaH2PO4, Na2HPO4, and Na3PO4 available. (Enter all numerical answers to three significant figures.) H3PO4(s) + H20(1) =H30+ (aq) + H2PO4 (aq) Kai = 6.9x10-3 H2PO4 (aq) + H20() = H30+(aq) + HPO42- (aq) Ka2 = 6.2x 10-8 HPO42-(aq) + H20(I) = H30+(aq) + PO43-(aq) Ka3 = 4.8 x 10-13 Which of the available chemicals...
A buffer with a pH of 3.92 contains 0.19 M of sodium benzoate and 0.36 M of benzoic acid. What is the concentration of [H3O+] in the solution after the addition of 0.054 mol HCl to a final volume of 1.7 L? Assume that any contribution of HCl to the volume is negligible. [H3O+] = M Allerede C., Calculate the change in pH when 7.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that...
You are instructed to create 400. mL of a 0.39 M phosphate buffer with a pH of 6.2. You have phosphoric acid and the sodium salts NaH2PO4, Na2HPO4, and Na3PO4 available. (Enter all numerical answers to three significant figures.) H3PO4(s) + H2O(l) = H30+ (aq) + H2P04 (aq) Kai = 6.9 x 10-3 H2PO4 (aq) + H20(1) =H30+ (aq) + HPO42-(aq) Ka2 = 6.2 x 10-8 HPO42-(aq) + H20(I) = H30+(aq) + PO43-(aq) Ka3 = 4.8 x 10-13 Which of...
A buffer solution contains 0.100 mol of HCIO and 0.100 mol of NaClO in 1.00 L. What is the pH of this buffer after 0.010 mol of NaOH are added? HCIO has a Ka = 3.0 x 10-8 07.61 8.47 7.52 O 6.57 7.43
(a) What is the pH of a solution that contains 0.100 M HClO and 0.300 M KClO? (b) If 50.00 mL of 0.100 M HCl is added to 1.00 L of the above buffer, what is the new pH? (b) If 50.00 mL of 0.100 M HCl is added to 1.00 L of the above buffer, what is the new pH?