Question

4.3b) Write a net ionic equation for the overall reaction that occurs when aqueous solutions of potassium hydroxide and carbonic acid (H₂CO₃) are combined.
Assume excess base. Use the pull-down boxes to specify states such as (aq) or (s)

4.3c) Write a net ionic equation for the reaction that occurs when solid zinc carbonate is combined with excess aqueous hydroiodic acid.

Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed leave it blank.

4.5a) A student weighs out 6.05 g of MgI₂, transfers it to a 125. mL volumetric flask, adds enough water to dissolve the solid and then adds water to the 125 mL mark on the neck of the flask.

Calculate the concentration (in molarity units) of magnesium iodide in the resulting solution?

4.5a2) In the laboratory, a student adds 16.8 g of manganese(II) bromide to a 500. mL volumetric flask and adds water to the mark on the neck of the flask. Calculate the concentration (in mol/L) of manganese(II) bromide, the manganese(II) ion and the bromide ion in the solution.

[MnBr2]=	M
[Mn2+] =	M
[Br-] =	M

4.5a3) Calculate the mass, in grams, of nickel(II) iodide that must be added to a 300-mL volumetric flask in order to prepare 300 mL of a 0.248 M aqueous solution of the salt.

4.5c) Calculate the volume (in mL) of 0.660 M HNO₃ needed to react completely with 6.28 g of NiCO₃ in a gas-forming reaction?

4.5d) Calculate the volume of 0.124 M sodium hydroxide required to neutralize 22.2 mL of a 0.220 M hydrochloric acid solution.

4.5d2) Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the unwieldy formula of KHC₈H₄O₄. This is often written in shorthand notation as KHP.
If 21.40 mL of a barium hydroxide solution are needed to neutralize 1.535 grams of KHP, what is the concentration (mol/L) of the barium hydroxide solution?

4.5e1) A 1.018-g sample of an unknown monoprotic acid is dissolved in water and titrated with standardized barium hydroxide. The equivalence point in the titration is reached after the addition of 33.68 mL of 0.1621 M barium hydroxide to the sample of the unknown acid. Calculate the molar mass of the acid.

4.5e2) The concentration of a SO₃^2- solution is determined by titrating it with a 0.1234 M solution of dichromate. The balanced net ionic equation for the reaction is shown below.

• Cr₂O₇^2-(aq) + 3 SO₃^2-(aq)+8 H₃O⁺(aq) -------> 2 Cr³⁺(aq) + 3 SO₄^2-(aq)+12 H₂O(l)

In one experiment, 20.49 mL of the 0.1234 M Cr₂O₇^2- solution is required to react completely with 30.00 mL of the SO₃^2- solution. Calculate the concentration of the SO₃^2- solution.