1. how can a 98% sulphuric acid be diluted to get a concentration of 0.05 mol per L?
1. how can a 98% sulphuric acid be diluted to get a concentration of 0.05 mol...
Determine the concentration of 20.0 mL of the sulphuric acid when 1.00 mol/L sodium hydroxide is used as the titrant.
how do you calculate pH of super concentrated acid (such as 98% sulphuric acid or 99,5% ethanol)?
If you digested 25 mg of pure ferrocene in nitric acid and then diluted the resulting solution up to 500 mL with 1% aqueous hydrochloric acid, what would be the concentration of iron in solution (provide an answer in both mg/L and mol/L)?
4. If you digested 25 mg of pure ferrocene in nitric acid and then diluted the resulting solution up to 500 mL with 1% aqueous hydrochloric acid, what would be the concentration of iron in solution (provide an answer in both mg/L and mol/L)?
Dundalk Institute of Technology Jan 2017 Question 4 000 ML (a) A 50.0 cm sample of sulphuric acid (H2504) was diluted to 1.00 Litre. A sample of the diluted sulphuric acid was analysed by titrating with aqueous sodiun hydroxide (NaOH) In the ttration, 25.0cm2 of 1.00 mol/ Laqueous sodium hydroxide required of the diluted sulphuric acid for neutralisation. 0 Write the equation for the full neutralisation of sulphuric acid by sodium ydroxide. (0)C (ili) Calculate the concentration(M) of the diluted...
1. Assume that 1.00 mol of HCOOH and 0.725 mol of HCOONa are diluted in an aqueous solution of 1.00 L of solution: a. Calculate the pH of the solution (Ka = 1.77 x 10-4) b. Assume that 0.10 mol of a strong acid such as HCl is added to the previous HCOOH / HCOONa solution. Calculate the pH of the new solution.
• Another student diluted her acetic acid sample with 10 ml of water before titrating with NaOH. Does this change the concentration of the acetic acid sample? Explain. • Does this change the pk, determined from the graph? 3. Look at all of your titration curves. Starting at 1 mL past the neutralization point, what can you say about all four graphs? 4. Use your concentration of acetic acid in mol/L and a density of 0.9987 g/mL for the acetic...
A buffer solution contains 0.05 mol of acetic acid and 0.065 mol of sodium acetate in 1.00-L. What is the pH of the buffer after the addition of 0.01 mol of HNO3? Ka(acetic acid) = 1.8 x 10^-5 Thank you!
Buffer action 4 A buffer solution consisting of 0.05 mol/L acetic acid (CH3COOH) and 0.05 mol/L acetate (CH3COO-) has been used to buffer a 1 L solution at pH 4.7. A small amount of sodium hydroxide solution containing 0.0001 mol NaOH was added. Which of the following reactions best represents the buffer action? + Select one: O a. NaOH(aq) Na+(aq) + OH(aq) O b. CH3COOH(aq) + H2O(1) CH3COO(aq) H30*(aq) O c. CH3COO(aq) + H2O(0) CH3COOH(aq) OH(aq) O d. CH3COOH(aq) +...
we consider an ammonium solution with a concentration of 0.05 mol / L 1) Write the equation of acidic basic equilibrium between NH4 + ammonium ions and water 2) Express literally the acidity constant KA of this equation. 3) Make the progress table showing the progress of the reaction x and give the expression of the acidity constant KA as a function of x. 4) Establish the second degree equation to determine the concentration of H3O + ions 5) Calculate...