2. Calculate the pH of a 0.4480 M solution of the base H2BO3-1 dissolved in water if Ka = 5.4x10-10 for H3BO3.
3. Calculate the pH of a solution containing the following compounds. (Note that these are concentrations before any reaction occurs).
[NaH2PO4] | 0.300 M |
[Na2HPO4] | 0.840 M |
[KOH] | 0.054 M |
4. For the titration of 15.00 mL of 0.100 M C6H5OH with 0.150 M NaOH, calculate the pH after the addition of 6.00 mL of NaOH.
2. Calculate the pH of a 0.4480 M solution of the base H2BO3-1 dissolved in water...
1. Calculate the pH of a 0.0820 M solution of the acid HClO dissolved in water if Ka = 2.9x10-8. 2. Calculate the pH of a 0.4480 M solution of the base H2BO3-1 dissolved in water if Ka = 5.4x10-10 for H3BO3. 3. Calculate the pH of a solution containing the following compounds. (Note that these are concentrations before any reaction occurs). [NaH2PO4] 0.300 M [Na2HPO4] 0.840 M [KOH] 0.054 M 4. For the titration of 15.00 mL of 0.100...
Calculate the pH of a solution containing the following compounds. (Note that these are concentrations before any reaction occurs). [NaH2PO4] 0.300 M [Na2HPO4] 0.840 M [KOH] 0.054 M
4.) For the titration of 15.00 mL of 0.100 M C6H5OH with 0.150 M NaOH, calculate the pH after the addition of 6.00 mL of NaOH. 5.) For the titration of 30.00 mL of 0.090 M HNO2 with 0.120 M NaOH, calculate the pH at the equivalence point.
1 . If a buffer solution is 0.260 M in a weak acid (?a=8.3×10−5)and 0.480 M in its conjugate base, what is the pH? pH= 2. If a buffer solution is 0.200 M in a weak base (?b=5.0×10−5) and 0.530 M in its conjugate acid, what is the ph 3. Phosphoric acid is a triprotic acid (?a1=6.9×10−3, ?a2=6.2×10−8 , and ?a3=4.8×10−13 To find the pH of a buffer composed of H2PO4 - (aq) ) and HPO4 2− (aq) , which...
Calculate the pH of a buffer solution that contains 0.56 M NaH2PO4 and 0.21M Na2HPO4 Calculate the change in pH if 0.050 g of solid NaOH is added to 200 mL of the solution in the problem above.
(ueak acid/shing base 3. Calculate the pH at the following points for the titration of 25.0 mL of 0.100 M formic acid (Ka-1.80 x 10") with 0.100 M NaOH: VNOH 0.00 mL, 15.00 mL, 25.00 mL, 40.00 mL. Draw a graph of pH vs. VaoH. (30 points) (b) Buffer capacity can be thought of as how well a solution resists changes in pH after a strong base/acid is added. A buffer is most effective to resisting pH changes when what...
1. You are titrating a 100.0 mL solution of 0.050 M HBrwith a 0.150 M solution of KOH. What will be the pH after the addition of 25.0 mL KOH? 2. You titrate 250 mL of 0.250 M acetic acid (Ka= 1.8 x 10-5) with 50.0 mL of 0.350 M NaOH. What is the pH of this solution? 3. For the titration in question 2, what would be the Kaof an ideal indicator.
Consider a solution formed by mixing 41.0 mL of 0.100 M H2SO4, 76.0 mL of 0.100 M HOCl, 25.0 mL of 0.200 M NaOH, 26.0 mL of 0.100 M Ba(OH)2, and 12.0 mL of 0.150 M KOH. Calculate the pH of this solution. (Refer to this table of Ka values of common monoprotic acids.) (with the correct sig figs)
7. Calculate the pH of the solution obtained by titrating 50.0 mL of 0.100 M HNO2(aq) with 0.150 M NaOH(aq) to the equivalence point. Take Ka = 5.6 x 10 - M for HNO2(aq).
1. The following graph is provided for the titration of 10.00 mL benzoic acid solution with a strong base. The concentration of NaOH is 0.100 M. A. Based on this graph given below, determine the Ka. B. Determine the molarity of the acid. Benzoic acid titration with 0.1 M NaOH 12.00 10.00 8.00 pH 6.00 4.00 2.00 0.00 0.00 5.00 10.00 15.00 Volume of NaOH mL