Titration Calculations - Page 5
Questions
- What volume of sodium hydroxide is required to titrate a #0.1*mol*L^-1# solution of acetic acid?
- You have a vinegar solution you believe to be 0.83 M. You are going to titrate 20.0mL of it with a NaOH solution that you know to be 0.519 M. At what volume of added NaOH solution would you expect to see the end point?
- A #15.62*mL# volume of monoprotic acid reached a stoichiometric endpoint with #16.49*mL# of sodium hydroxide whose concentration was #1.175*mol*L^-1#. What is the concentration of the acid?
- Using the correct amount of significant figures, how many milliliters of 8.48×10^(−2) M Ba(OH)2 (aq) are required to titrate 54.90 mL of 5.38×10^(−2) M H(NO)3?
- A solution of sodium hydroxide is standardized against potassium hydrogen phthalate. From the following data, calculate the molarity of NaOH solution? (See details below)
- What do we mean by #"back titration"#?
- How do you use titration calculations to find pH?
- How does titration affect molarity?
- In a titration of 0.35 M HCl and 0.35 M NaOH, how much NaOH should be added to 45.0 mL of HCl to completely neutralize the acid?
- What is the technique you would use to separate and collect hydrated copper (ll) sulfate, #"CuSO"_4cdot5"H"_2"O"# from its aqueous solution?
- 29.4mL of an #CH_3COOH# solution were titrated with 18.5mL of a 0.175M #LiOH# solution to reach the equivalence point What is the molarity of the #CH_3COOH# solution?
- Why are titration problems done with vigorous swirling?
- What is the pH when 25.00 mL of 0.20 M CH3COOH has been titrated with 40.00 mL of 0.10 M NaOH?
- How do you do titration problems involving pH?
- What volume of 1 M sulfuric acid is needed to titrate a 12 ml sample of 0.45 M NaOH?
- What is the molarity of the potassium permanganate solution?
- 3.6 #g# of oxalic acid (#H_2C_2O_4 * 2H_2O#) are dissolved and the volume is made upto 150 #ml#. Calculate the normality of the solution for redox titration?
- Consider the titration of 300.0 mL of #0.300 MNH_3 (K_b = 1.8 xx 10^-5)# with #0.300 M HNO_3#. What is the pH at the equivalence point?
- What is the pH at the half equivalence point when 50.0 mL of 0.200 M NaOH is titrated with 0.100 M HCl? The starting pH is 13.3.
- How do you solve titration problems for pH?