a solution is prepared by combining the following: 200mL .1 M H2SO4 100mL .2 M NaOH 700mL .143 M K2SO4 The pH of the solution = 3.6 What is the Ka of HSO4?
a solution is prepared by combining the following: 200mL .1 M H2SO4 100mL .2 M NaOH...
A buffer solution is prepared by combining 750.0 ml of 1.00 M of ammonia and 250 ml of 1.00 M ammonium chloride. What is the pH of the buffer? ( Ka of NH4+=5.6*10^-10, Kb of NH3= 1.8*10^-5)
A buffer solution is prepared by combining 750.0 ml of 1.00 M of ammonia and 250 ml of 1.00 M ammonium chloride. What is the pH of the buffer? ( Ka of NH4+=5.6*10^-10, Kb of NH3= 1.8*10^-5)
A 1.32 L buffer solution consists of 0.121 M butanoic acid and 0.345 M sodium butanoate. Calculate the pH of the solution following the addition of 0.066 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The Ka of butanoic acid is 1.52 × 10-5. A 1.44 L buffer solution consists of 0.326 M propanoic acid and 0.103 M sodium propanoate. Calculate the pH of the solution following the addition of...
If 100mL of 0.10M CH3COOH (Ka=1.8x10-5) is titrated with 0.10 M NaOH. Calculate the pH value for the following solution. A. 75.0 mL of NaOH is added B. 100.0 mL of NaOH is added C. Suggest an indicator for this titration
Find the concentration (molarity) of an aqueous solution prepared by dissolving 10g of NaOH(s) in 100mL of water. Find the concentration (molarity) of a NaOH solution that contains 5g of NaOH and 1000 mL of water. What is the new concentration when we add 1L more of water to the prepared solution in question (2).? If you have 10 ml of a 5M solution of NaOH, how many mol of NaOH you have? How many mol of Na+ you have?...
What is the pH of an aqueous solution made by combining 41.20 mL of a 0.4608 M ammonium chloride with 45.82 mL of a 0.3866 M solution of ammonia to which 3.070 mL of a 0.0838 M solution of NaOH was added? What is the pH of an aqueous solution made by combining 41.56 mL of a 0.4057 M sodium formate with 45.00 mL of a 0.3759 M solution of formic acid? What is the pH of an aqueous solution...
1. A solution is prepared by dissolving 0.23 mol of butanoic acid and 0.27 mol of sodium butanoate in water sufficient to yield 1.00 L of solution. The addition of 0.0O5 mol of HCI to this buffer solution causes the plH to drop slightly. The pH does not decrease drastically because the HCl reacts with the present in the buffer solution. The Ka of butanoic acid is 1.36x 10-3 A) H20 в) Нзо+ butanoate ion D butanoic acid AlE) This...
3. A solution is prepared by treating 50 mL of 0.50 M HF (Ka = 6.6x10 ) with 10 mL of 1.15 M NaOH. Calculate the pH of the solution. 4. If enough NaOH is added to the solution in problem 3 to neutralize the HF, what will the pH be? 5. 42.16 mL of a solution of NaOH are required to neutralize 0.7878 g of potassium hydrogen phthalate (Mwt = 204.23 g/mol). Calculate the molar concentration of NaOH in...
1. You are titrating a 100.0 mL solution of 0.050 M HBrwith a 0.150 M solution of KOH. What will be the pH after the addition of 25.0 mL KOH? 2. You titrate 250 mL of 0.250 M acetic acid (Ka= 1.8 x 10-5) with 50.0 mL of 0.350 M NaOH. What is the pH of this solution? 3. For the titration in question 2, what would be the Kaof an ideal indicator.
a) What is the pH of a solution that consist of 0.20 M ammonia, NH3, and 0.20 M ammonium choride, NH4Cl? (Kb for ammonia is 1.8 x 10-5) b) 1.25 g of benzoic acid (C6H5CO2H) and 1.25 g of sodium benzoate (NaC6H5CO2) are dissolved in enough water to make 250 mL solution. Calculate the pH of the solution using the Handerson-Hasselbach equation (Ka for benzoic acid is 6.3 x 10-5). c) What is the pH after adding 82 mg of...