45.00 mL of a 0.250 M H2SO4 solution is titrated with 0.100 M NaOH. a. What is the chemical equation that describes this neutralization reaction? b. What is the volume in mL of NaOH required to reach the equivalence point? c. At the equivalence point, what are the sodium and sulfate ion concentrations? d. At the equivalence point, what are the pH and pOH
Determine the final volume (mL) for each of the following. Part A: Diluting 56.5 mL of a 11.5 M NH4Cl solution to give a 5.00 M NH4Cl solution? Part B: Diluting 25.0 mL of a 11.5 M NaNO3 solution to give a 2.00 M NaNO3 solution. Part C: Diluting 7.50 mL of an 16.0 M H2SO4 solution to give a 2.50 M H2SO4 solution. Part A Diluting 56.5 mL of a 115 MNH,CI solution to give a 500 MNH,CI solution...
100. mL of 0.200 MHCl is titrated with 0.250 M NaOH. Part A What is the pH of the solution at the equivalence point? Express the pH numerically. View Available Hintis)
How many mL of 0.250 M BaCl2 would you need to precipitate all the sulfate ion present in 38.1 mL of 0.197 M H2SO4 solution? What is the concentration (M) of the chloride ion remaining in the resulting solution?
6. How many mL of a 0.250 M KCl solution contains 34.5 g KCI? 7. To what volume (in mL) should you dilute 100.0 mL of a 2.50 M CaCl2 solution to obtain a 0.550 M CaCl2 solution?
(0) How many milliers of 0.155 M HCl are needed to neutralize completely 45.0 ml of 0.101 M Ba(OH)2 solution? ml (b) How many milliliters of 2.50 M H2SO4 are needed to neutralize 25.0 9 of NaOH? (c) If 54.8 ml of BaCl solution is needed to precipitate all the sulfate in a 544 mg sample of Na2SO4 (forming Basod), what is the molarity of the solution? (d) If 37.5 mL of 0.250 M HCl solution is needed to neutralize...
(a) How many milliliters of 0.155 M HCl are needed to neutralize completely 35.0 mL of 0.101 M Ba(OH)2 solution? (b) How many milliliters of 2.50 M H2SO4 are needed to neutralize 75.0 g of NaOH? (c) If 56.8 mL of BaCl2 solution is needed to precipitate all the sulfate in a 554 mg sample of Na2SO4 (forming BaSO4), what is the molarity of the solution? (d) If 47.5 mL of 0.250 M HCl solution is needed to neutralize a...
50.0 mL of a 0.250 M AgNO3 solution and 50.0 mL of 0.400 M Na2CO3 solution are mixed. How much of the silver carbonate precipitate will be formed? 2 AgNO3 (aq) + Na2CO3 (aq) -> Ag2CO3 (s) + 2 NaNO3 (aq)
When preparing 150.0 mL of a 0.250 M solution of Ca(OH)2 from a 4.9 M stock solution how much of the stock solution (in mL) do you need to add? Record to the appropriate amount of significant figures.
Consider the titration of a 21.0 – mL sample of 0.105 M HC2H3O2 with 0.125 M NaOH. Determine each of the following. Part A the initial pH Part B the volume of added base required to reach the equivalence pointPart C the pH at 4.00 mL of added basePart D the pH at one-half of the equivalence point Part E the pH at the equivalence point