A solution of hydrocyanic acid is prepared by dissolving 0.10 mol HCN in enough water to make 1.0 L of solution. If 0.0050 mol of NaCN is added to the solution with no increase in volume, what is the concentration of H+ when equilibrium is re-established? Use concentrations to get equilibrium constant. CN ions added and used Na+ as a spectator ion.
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- Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.Consider the titration of butyric acid (HBut) with sodium hydroxide. In an experiment, 50.00 mL of 0.350 M butyric acid is titrated with 0.225 M NaOH. Ka HBut=1.5105. (a) Write a balanced net ionic equation for the reaction that takes place during titration. (b) What are the species present at the equivalence point? (c) What volume of sodium hydroxide is required to reach the equivalence point? (d) What is the pH of the solution before any NaOH is added? (e) What is the pH of the solution halfway to the equivalence point? (f) What is the pH of the solution at the equivalence point?
- A buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M nitrous acid, HNO2. Assume no volume change after HNO2 is dissolved. Calculate the pH of this buffer.A solution of hydrocyanic acid is prepared by dissolving 0.10 mol HCN in enough water to make 1.0 L of solution. If 0.0050 mol of NaCN is added to the solution with no increase in volume, what is the concentration of H+ when equilibrium is re-established? The pH of the solution is 5.2 before adding 0.005 mol NaCN. (Hint: Use concentrations to get equilibrium constant. Account for the added CN- ions. Treat Na+ is a spectator ion) *final answer in 4 decimalsA solution of hydrocyanic acid is prepared by dissolving 0.10 mol HCN in enough water to make 1.0 L of solution. If 0.0050 mol of NaCN is added to the solution with no increase in volume, what is the concentration of H+ when equilibrium is re-established? The pH of the solution is 5.2 before adding 0.005 mol NaCN. (Hint: Use concentrations to get equilibrium constant. Account for the added CN- ions. Treat Na+ is a spectator ion)
- 1. You are taking samples at a contaminated mine site from a carbonate aquifer to determine the concentration of dissolved lead in the sample. To preserve the sample, you acidify it to pH 5. How much HCl, in equivalents/L, must be added to this sample to make it pH 5 if the total carbonate concentration is 102 M and the initial pH is 10? Note that the total carbonate is the sum of all of the carbonate species ([H2CO3]+[HCO3] + [CO2]) present in the sample. What are the acid-base pairs responsible for buffering in this sample?A buffer is made by adding 0.68 g of sodium formate, NaHCOO (molar mass = 68.0 g/mol), to 1.00 L of 0.015 M formic acid, HCOOH (K a = 1.8 × 10−4). The pH of the buffer is 3.57. What will the pH be after 10.0 mL of 0.50 M HCl(aq) is added to the buffer? I know how to solve it, I just don't know what the equation of the buffer is supposed to look like. I have HCOO- <---> HCl + HCOOH, but I don't think that's right. Thank you!Consider a hypothetical sparingly soluble salt of the form A(OH)2. A 20.00 mL saturated, purely aqueous solution of this salt was reacted with 4.35 mL of 0.15 M HCl solution for the complete neutralization of the OH- ions. Calculate the equilibrium molar concentration of hydroxide ions in the saturated solution of A(OH)2.
- A buffer solution contains 0.351 M KHSO3 and 0.344 M K2SO3.If 0.0252 moles of hydroiodic acid 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 hydroiodic acid)pH =A buffer solution contains 0.254 M NaHSO3 and 0.348 M Na2SO3. If 0.0285 moles of hydroiodic acid are added to 250 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume change does not change upon adding hydroiodic acid)A buffer is prepared by adding 10.0 g of ammonium chloride(NH4Cl) to 250 mL of 1.00 M NH3 solution. (a) Whatis the pH of this buffer? (b) Write the complete ionic equationfor the reaction that occurs when a few drops of nitricacid are added to the buffer. (c) Write the complete ionicequation for the reaction that occurs when a few drops ofpotassium hydroxide solution are added to the buffer.