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General Chemistry: Atoms First
- An important component of blood is the buffer combination of bicarbonate ion and carbonic acid. Consider blood with a pH of 7.42. a What is the ratio of [H2CO3] to [HCO3]? b What does the pH become if 15% of the bicarbonate ions are converted to carbonic acid? c What does the pH become if 25% of the carbonic acid molecules are converted to bicarbonate ions?arrow_forwardConsider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?arrow_forwardA friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?arrow_forward
- Identify the buffer system(s)the conjugate acidbase pair(s)present in a solution that contains equal molar amounts of the following: a. HF, KC2H3O2, NaC2H3O2, and NaF b. HNO3, NaOH, H3PO4, and NaH2PO4arrow_forwardA buffer is prepared in which the ratio [ H2PO4 ]/[ HPO42 ]is 3.0. (a) What is the pH of this buffer? (b) Enough strong acid is added to convert 15% of HPO42- to H2PO4-. What is the pH of the resulting solution? (c) Enough strong base is added to make the pH 7.00. What is the ratio of [H2PO4-] to [HPO42-] at this point?arrow_forwardAn important component of blood is the buffer combination of dihydrogen phosphate ion and the hydrogen phosphate ion. Consider blood with a pH of 7.44. a What is the ratio of [H2PO4] to [HPO42]? b What does the pH become if 25% of the hydrogen phosphate ions are converted to dihydrogen phosphate ion? c What does the pH become if 15% of the dihydrogen phosphate ions are converted to hydrogen phosphate ions?arrow_forward
- Write the net ionic equation in which the slightly soluble salt barium fluoride, BaF2, dissolves in dilute hydrochloric acid.arrow_forwardCalculate the pH at the following points in a titration of 40.0 mL of 0.100 M barbituric acid(Ka = 9.8 × 10−5) with 0.100 M KOH. (a) no KOH added (b) 20.0 mL of KOH solution added (c)39.0 mL of KOH solution added (d) 40.0 mL of KOH solution added (e) 41.0 mL of KOHSketch an appropriate pH titration curve indicating the buffer region, equivalence point,and excess base region. Why is the pH at the equivalence point not 7.00?arrow_forwardAssume you titrate 20.0 mL of 0.11 M NH3 with 0.10 M HCl. (a) What is the pH of the NH3 solution before the titration begins? (b) What is the pH of the equivalence point? (c) What is the pH at the midpoint of the titration? (d) Which indicator would you suggest to detect the equivalence point? (e) Calculate the pH of the solution after adding 5.00, 11.0, 15.0, 20.0, 22.0, and 25.0 mL of the acid. Combine this information with that from (a) through (c) and plot the titration curve.arrow_forward
- 11. Buffer X contains 8.0 mmol of NH3 and 8.0 mmol of NH. Buffer Y contains 20.0 mmol of NH3 and 20.0 mmol of NH. Which of the following statements is TRUE? (a) Buffer X will have a pH five times more than Buffer Y. (b) Buffer X will have a pH five times less than Buffer Y (c) Buffer X and Buffer Y will have the same pH (d) Buffer X and Buffer Y cannot be compared unless we have the pKa of NHarrow_forwardThe major component of vinegar is acetic acid, CH3COOH. Its Ka is 1.8 × 10-5 . One student used 1.000 M NaOH to titrate 25.00 mL vinegar. At the end point, 21.82 mL NaOH was used. (a) What is the concentration of CH3COOH in vinegar? (b) What is the pH of the solution at the end point? (c) What indicator(s) the student should use in this titration? Explainarrow_forwardConsider the titration of formic acid, HCHO2, with barium hydroxide. (a) Write a balanced net ionic equation for the reaction. (b) Calculate K for the reaction. (c) Is the solution at the equivalence point acidic, basic, or neutral? (d) What would be an appropriate indicator for the titration?arrow_forward
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