A buffer solution is prepared by mixing equal concentrations of HClO(aq) and KClO(aq). A small amount of hydronium ion is added to the mixture. Write the chemical equation that illustrates how the buffer system removes the hydronium ion. Include the states in the reaction.
How it removes hydronium ion is as follows:
KClO(aq) => K+(aq) + ClO-(aq)
ClO-(aq) + H3O+(aq) => HClO(aq) + H2O(l)
NOTE: the HClO(aq) produced upon addition of H3O+ is a WEAK acid and will not ionize much, thus essentially removing the H3O+.
A buffer solution is prepared by mixing equal concentrations of HClO(aq) and KClO(aq). A small amount...
A buffer solution is made that is 0.455 M in HClO and 0.455 M in KClO. (1) If Ka for HClO is 3.50×10-8, what is the pH of the buffer solution? (2) Write the net ionic equation for the reaction that occurs when 0.102 mol HCl is added to 1.00 L of the buffer solution. Use H3O+instead of H+.
Suppose that a small amount of HCl is added to a buffer solution containing HF(aq) and NaF(aq). What change will occur to the buffer solution? The concentration of fluoride ion will decrease and the concentration of hydrogen fluoride will increase. The concentration of fluoride ion will increase, and the concentration of hydrogen fluoride will decrease. The concentration of hydronium ion will decrease. The concentration of fluoride ion will increase, and the concentration of hydrogen fluoride will increase.
You prepared a phosphate buffer solution by mixing 40.0 mL of 0.250 M KH_2PO_4 and 60.0 mL ol 0.450 M K_2HPO_4 solution. (a) What are the molar concentrations of H_2PO_4 and HPO_4^2-, respectively, in the final buffer solution? (b) Calculate the pH of the solution. (c) Write a net ionic equation when a strong acid, such as HCl(aq) is added to the phosphate buffer solution. (d) Calculate the final pH when 0.0060 mol of HCl is added to the buffer...
For the following buffer system: a. Calculate the concentrations of the major species present in a buffer solution prepared by mixing 12.5g of sodium acetate (NaCH3CO2, a salt) in 325mL of 1.5M acetic acid (CH3CO2H(aq), a weak acid). Ka,CH3CO2H = 1.8x10-5 . b. Write out the acid-base reaction of this solution and identify the conjugate acid base pairs. c. Calculate the pH of this acidic buffer solution. d. By how much would the pH of the solution change if 10.0mL...
Consider the buffer solution: HNO2(aq) + H2O(l) + NO2 (aq) +H30+(aq) What happens to the concentrations of HNO2 and NO2 when a small amount of acid is added to the solution?
Consider the buffer solution: HNO3(aq) + H2O(1) - NO2 (aq) +H30*(aq) What happens to the concentrations of HNO2 and NO2 when a small amount of acid is added to the solution?
I need help with both answers. Thank you.
< Question 29 of 65 > A buffer is prepared by mixing hypochlorous acid (HCIO) and sodium hypochlorite (Nacio). If a strong acid, such as HCl, is added to this buffer, which buffer component neutralizes the additional hydrogen ions (H)? CIO OHCIO. Write a balanced chemical equation for the reaction of the selected buffer component and the hydrogen ion (H+). Do not include physical states. chemical equation:
Consider the buffer solution: HNO3(aq) + H20(1) -- NO2 (aq) + H30*(aq) What happens to the concentrations of HNO2 and NO2 when a small amount of acid is added to the solution?
Consider the buffer solution: HNO2(aq) + H2O(l) + NO2 (aq) + H30+(aq) • What happens to the concentrations of HNO2 and NO2 when a small amount of acid is added to the solution?
Calculate the pH of a buffer solution prepared by mixing 75 mL of 1.0 M lactic acid and 25 mL of a 1.0M sodium lactate. (pka of lactic acid = 3.86) Calculate the change in pH that occurs when 0.01moles of OH are added to a 1L buffered solution that contains 0.5M acetic acid (HC_2H_3O_2) and 0.5M acetate ion (C_2H_3O_2). Acetic acid pka = 4.76.