10) A buffer solution with a volume of 775.0 mL is made with 0.225 mol of HC;H;O2 and 0.100 mol NaC2H3O2. If 2.30 g of NaOH is added without changing the volume of the solution, what is the pH of the resulting solution? The pk, of acetic acid is: 4.74. (4.71)
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- 6. (13 pts) A solution of 0.1000 M HCl was used to titrate 25.00 mL of Na2CO3 (0.0800 M). Calculate the pH of the solution when adding following amount of HCI. For H2CO3 = Ka2 4.69 x 10-11 Kal = 4.46 × 10-7 a) 0.00 mL (before the titration) b) 5.00 mL c) at the first equivalent point d) 45.00 mL10) A buffer solution with a volume of 775.0 mL is made with 0.225 mol of HC2H3O2 and 0.100 mol NaC2H3O2. If 2.30 g of NaOH is added without changing the volume of the solution, what is the pH of the resulting solution? The pKa of acetic acid is: 4.74. (4.71)(5.7: Similar to For practice 5.11)The titration of a 20.0 mL sample of an H₂SO4 solution of unknown concentration requires 18.88 mL of a 0.203 M KOH to reach the equivalence point. What is the concentration (in M) of the unknown H₂SO4 solution? (Hint: Write the balanced reaction equation first.) O 0.0958 M O 0.383 M O 0.767 M O 0.192 M
- (10.2) Calculate the fluoride ion concentration and pH of a solution that is 0.20 M in HF and 0.10 M in HCl. Ka 6.8 × 10¬4A 250.00 mL solution of 0.00215 M AB4 is added to a 230.00 mL solution of 0.00380 M C3D2. What is pQsp for A3D4? Answer: (18.607)7. (8 pts) Calculate the solubility product, Ksp, for SrF2, given that its solubility is 0.0080 g per 225.0 mL of solution. SrF (s) Sr2 (aq) 2F (aq) 2
- Citric acid/citrate buffer is a pH buffer that is used for baby locations. A pH buffer is prepared by dissolving 17.77 grams C6H5O7Na2 and 19.67 grams of C6H4O7Na3 in enough water to make 250.0 mL solution. C6H40 (aq) + H30¹ (1) C6H₂O² (aq) + H₂O(1) The 3rd acid dissociation constant of citric acid is 4.012×10-7. Please answer the following questions. A. B. What is the pH of the solution? pH = Please provider your answer below. 0² If you add 5.000 mL, 0.5363 M of HC1 to 250.0 mL above solution you prepared, what will be the final pH? Assume that the volume is additive. pH = Please provider your answer below. 00 → → $ □ C. If you add 5.000 mL, 0.5363 M of Ba(OH)₂ to 250.0 mL above solution you prepared, what will be the final pH? Assume that the volume is additive. pH = Please provider your answer below. → → $ $Comparing the two quantities based on the given condition, which is greater I or II? or are they equal? Can the quantities be compared? Ten (10) mL of solution X contains 0.100 M HCl and 0.100 M HA (pKa = 5) Ten (10) mL of solution Y contains 0.100 M HCl and 0.100 M HB (pKa = 7) Both solutions are titrated with 0.100 M NaOH. I. Volume of titrant required to reach the 2nd equivalence point in solution X II. Volume of titrant required to reach the 2nd equivalence point in solution Y.A buffer made up of equal volumes (403.6 mL) of each of 0.828 M A H and 0.898 M A minus. What is p H of the buffer after addition of 11.42 mL of 0.238 M N a O H? K a of A H is 6.910E-5. Answer: (4.203)
- Q1 H2CO3 - HCO, Carbonic anhydrase co,dissolves in plasma Carbonic acid Bicarbonate co, combines with hemoglobin co HOH,Co, HHCo Ho combines with hemogiobin ion CH Hčo,- Plasma Red blood cells The pk, of carbonic acid is 6.35. A solution is made by combining 50 mL 1.0 M carbonic acid, 2.0 mL of 5.0 M KOH and 448 mL pure water (assume the total volume is 500 mL). Calculate the pH of the resulting solution. Do we live or die or are we just ill? Blood pH Levels Death Acidosis Normal pH Alkalosis Death 7 7.35 7.45 7.8(3) 11. In a titration it is found that 97.7 mL of 0.154 M NaOH(aq) is needed to neutralize 25.0 mL of a solution of HCl(aq). Calculate the concentration of the HCl solution. Show your work. [Hint: Write a balanced equation for the reaction first.]Indicate the concentration of each ion present in the solution formed by mixing the following. Assume that the volumes are additive. Enter your answers, separated by a comma, using three significant figures. (1.) 42.0 mL of 0.140 M NaOH and 37.6 mL of 0.430 M NaOH. (2.) 44.0 mL of 0.150 M Na2SO4 and 25.0 mL of 0.200 M KCl (3.) 3.10 g KCl in 75.0 mL of 0.270 M CaCl2