Calculate the equilibrium constant (Ka) for this acid.

O D. K = 1 OE K 1 QUESTION 25 A solution is prepared by adding 0.10 mol of iron(III) chlorite, Fe(CIO)3, to 1.00 L of water. Which statement about the solution is correct Periodic table.pdf OA. The solution is basic. O B. The solution is neutral. OC. The solution is acidic. O D. The values of Ka and Kb for the species in solution must be known before a prediction can be made. Type here to search e も DOLL

b. I'm falling asleep.... The CO₂ concentration in a classroom can increase over the lecture period due to poor ventilation. You decide to measure the pH of pure water in contact with the atmosphere as an indirect way to determine whether you have adequate ventilation. You measure a pH value of 5.3. Assuming equilibrium, i. What is the concentration of CO2 in the classroom? ii. How does the value you calculated compare to the recommended safe level of 800-1000 ppm?

Which of the following statement best explain why the acidity of carboxylic acids is greater than those of the alcohols? a. Alcohols behave as neutral compounds in aqueous solution. b. Alcohol has the ability to donate proton to becomes a negative ion called an alkoxide ion, RO– c. When a carboxylic acid donates its proton, it becomes a negatively charged ion, RCOO−, called a carboxylate ion which is more stabilized by resonance. d. The OH group in alcohol is less charged and often more difficult to release electron for chemical reactions.

23. Consider a generic polyprotic acid H2YO3. What is an appropriate combination of acid dissociation constants for this acid? Kal Ka2 A. 2.1 x 104 8.9 x 10-5 В. 3.2 х 10-6 2.2 x 10-10 С. 4.5 х 10-10 6.7 x 10-6 D. 5.3 x 10-5 1.8 x 10-4

A 0.121 M solution of acetic acid has a pOH of 11.20. What is the Ka of acetic acid? Oa. 2.5 x 10-6 Ob. 2.1 x 10-5 Oc. 3.3 x 10-22 Od. 1.6 x 103 Oe. 1.3 x 102

A. What is the Kb when the Ka of a solution is 5.47x10^-4? B. the Ka of an acid is determined to be 0.00589. What is the Pka? C. A solution is made where 0.878 moles HCl is added to water that has a total volume of 1855mL. what is the PH of the solution?

18.   A. Calculate [OH−] for this strong base solution: 7.3×10−2 M KOH and then it's pH   B. Calculate [OH−] for this strong base solution: 10.0 mL of 1.00×10−2 M Ca(OH)2 diluted to 500.0 mL and it's pH   C. Calculate [OH−] for the strong base solution formed by mixing 10.0 mL of 1.50×10−2 M Ba(OH)2 with 34.0 mL of 6.0×10−3 M NaOH and it's pH

Consider a solution of Hydrofluoric acid at equilibrium as follows:HF (aq)+H2O (l) F ̄ (aq)+H3O+ (aq) a.Suppose a strong base (OH-) is added to the buffer system above. Which two species could react and why? b.Write the chemical reaction for the reaction of hydroxide ion (OH-) being neutralized by reacting with the hydrofluoric acid. c.Explain why the addition of a small amount of strong base will not cause a significant change in the pH of the solution as long as the HF is not used up. d. Suppose a strong acid (H3O+) is added to the buffer system above. Which species could react and why? e.Write the chemical reaction for the reaction of hydronium ion (H3O+) being neutralized by reacting with the fluoride ion. f.Explain why the addition of a small amount of strong acid will not cause a significant change in the pH of the solution as long as the fluoride ion (F ̄) is not used up.

Calculate the pH of a solution that is 0.70 M in HF ( Ka= 7.2 × 104) and 0.66 M in NaF. а. 3.40 O b.0.12 О с. 3.26 O d. 10.74 О е. 3.12