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- A 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?Consider a solution prepared by mixing a weak acid HA. HCl, and NaA. Which of the following statements best describes what happens? a. The H+ from the HCl reacts completely with the A from the NaA. Then the HA dissociates somewhat. b. The H+ from the HCl reacts somewhat with the A from the NaA to make HA, while the HA is dissociating. Eventually you have equal amounts of everything. c. The H+ from the HCl reacts somewhat with the A from the NaA to make HA while the HA is dissociating. Eventually all the reactions have equal rates. d. The H+ from the HCl reacts completely with the A from the NaA. Then the HA dissociates somewhat until too much H+ and A are formed, so the H+ and A react to form HA, and so on. Eventually equilibrium is reached. Justify your choice, and for choices you did not pick, explain what is wrong with them.You have a solution of the weak acid HA and add some HCl to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
- For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.Chloroacetic acid, HC2H2ClO2, has a greater acid strength than acetic acid, because the electronegativity chlorine atom pulls eloectroms way from the O-H bond and thus weakens it. What is the pH of a 0.045 M aqueous solution of chloroacetic acid? The Ka for HF is 1.3x10-3. You must solve the quadric equation for this problem. Express your answer to two decimal places. -------------------------------------------------------------------------------------------------------------------------- What is the pH of a 0.080 M aqueous solution of methylamine, CH3NH2? The Kb for methylamine is 4.4x10-4. You must solve the quadric equation for this problem. Express your answer to two decimal places.A students mistakenly titrates 25.0 mL of a 0.20 M H2SO4 solution, with 62.0 mL of a 0.15 M NaOH solution. What is the resulting pH?
- The concentration of CH3COOH (pKa=4.75) in vinegar is about 1.0 M. With this what do you predict the pH of vinegar to be?When 14.08 mL of 0.1594 M NaOH is added to 25.00 mL of 0.1235 M HX (an unknown weak acid), the resulting pH is 4.7. What is the Ka of the unknown acid?4. How many grams of CH3COONa must be added to 1.00 L of a 0.100 M CH3COOH solution in order for the pH of the solution to be 4.42?