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- A buffer solution contains 0.455 M ammonium chloride and 0.214 M ammonia. If 0.0538 moles of sodium hydroxide are added to 225 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume change does not change upon adding sodium hydroxide) pH = Submit Answer Retry Entire Group 9 more group attempts remainingA buffer solution contains 0.327 M acetic acid and 0.402 M sodium acetate. If 0.0258 moles of hydrobromic acid are added to 125 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume change does not change upon adding hydrobromic acid) pH = Submit Answer Retry Entire Group 9 more group attempts remainingA buffer solution contains 0.398 M KH₂PO4 and 0.355 M Na₂HPO4 If 0.0248 moles of hydrochloric acid are added to 150 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume change does not change upon adding hydrochloric acid) pH = Submit Answer Retry Entire Group 9 more group attempts remaining
- Determine the pH change when 0.112 mol HNO3 is added to 1.00 L of a buffer solution that is 0.398 M in HCIO and 0.397 M in Clo™. pH after addition - pH before addition = pH change = Submit Answer Retry Entire Group 7 more group attempts remainingWhat is the number of moles of 10.0 g NH₄Cl? What is the molar concentration of NH₄Cl? What is the pH of the buffer solution?Determine the pH change when 0.073 mol NaOH is added to 1.00 L of a buffer solution that is 0.351 M in HCIO and 0.397 M in CIO. pH after addition - pH before addition = pH change = Submit Answer Retry Entire Group 3 more group attempts remaining
- When 1.0 mL of 1.0 M HCl is added to 50. mL of a buffer solution that is 1.0 M in HC2H3O2 and 1.0 M in NaC2H3O2, the [H+] changes from 1.8 x 10-5 M to 1.9 x 10-5 M. Calculate the initial pH and the pH change in the solution. Initial pH: pH change:Determine the pH change when 0.061 mol HCI is added to 1.00 L of a buffer solution that is 0.357 M in CH3COOH and 0.222 M in CH3COO™. pH after addition - pH before addition = pH change = Submit Answer Retry Entire Group 9 more group attempts remaining4. A pH buffer solution contains 1.383 mole CH3COOH and 1.875 mole CH3COONa. The volume of the pH buffer solution is 250.0 mL. The acid dissociation constant of CH3COOH is 1.799x10-5. Please answer the following questions. A B. C. What is the pH of the solution? pH = Your answer follows. If you add 5.000 mL, 1.431 M of HCl to 250.0 mL above solution you prepared, what will be the final pH? Assume that the volume is additive. Your answer follows. If you add 5.000 mL, 1.431 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.
- Consider the buffer system of carbonic acid (H₂CO₂) and its salt, KHCO₂, which provides the conjugate base, HCO,. H_COjlog) + HJO W 7 HyO" loạ) + HCOy loa) How does the buffer react when some base is added? The bicarbonate ion (HCO) of the buffer reacts with the base. OHCO and H₂CO, both react with the base. O The buffer does not react. O The carbonic acid (H₂CO₂) of the buffer reacts with the base Question 15 Indicate whether each of the following reactions is an example of reaction of an acid with a metal, reaction of an acid with a carbonate, or acid-base neutralization reaction using the dropdown on the right. Reaction A: ZnCO3(s) + 2HBr(aq) → ZnBr₂(aq) + CO₂(g) + H₂O(l) Reaction B: Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g) HCI(g) + NaHCO3(s)→ NaCl(aq) + CO₂(g) + H₂O(0) H₂SO4(aq) + Mg(OH)2(s)→ MgSO4(aq) + 2H₂O(1) 3LIOH(aq) + H₂PO₂(aq) → Li₂PO₂(aq) + 3H₂O(0) Cal(s) + H₂SO4(aq) → H₂(g) + CaSO₂(aq) Reaction C: Reaction D: Reaction E: Reaction EA buffer solution is made that is 0.449 M in H₂S and 0.449 M in NaHS. If Ka1 for H₂S is 1.00 x 10-7, what is the pH of the buffer solution? pH = Use the References to access important values if needed for this question. Write the net ionic equation for the reaction that occurs when 0.093 mol HBr is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of H+) + Submit Answer + Retry Entire Group 8 more group attempts remainingWhich of the following aqueous solutions are good buffer systems? O0.19 M hydrocyanic acid + 0.16 M potassium cyanide 0.23 M hydrochloric acid + 0.15 M sodium chloride 0.37 M calcium bromide + 0.24 M potassium bromide 0.35 M ammonia + 0.30M barium hydroxide O 0.13 M calcium hydroxide + 0.22 M calcium chloride Submit Answer Retry Entire Group 9 more group attempts remaining
