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Chapter 4: Q4.7P (page 178)
Why are some ionic compounds soluble in water and others are not?
ANSWER:
Those ionic compounds which have a strong ionic bond, does not soluble in water.
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A mixture of CaCO3 and CaO weighing 0.693 g was heated to produce gaseous CO2. After heating, the remaining solid weighed 0.508g. Assuming all the CaCO3 broke down to CaO and CO2, calculate the mass percent of CaCO3 in the original mixture.
Question: State a general equation for a neutralization reaction.
On a lab exam, you have to find the concentrations of the monoprotic (one proton per molecule) acids HA and HB. You are given 43.5mL of HA solution in one flask. A second flask contains 37.2mL of HA, and you add enough HB solution to it to reach a final volume of 50.0mL. You titrate the first HA solution with 87.3mL of 0.0906M NaOH and the mixture of HA and HB in the second flask with 96.4mL of the NaOH solution. Calculate the molarity of the HA and HB solutions.
An unknown amount of acid can often be determined by adding an excess of base and then “back-titrating” the excess. A 0.3471-g sample of a mixture of oxalic acid, which has two ionizable protons, and benzoic acid, which has one, is treated with 100.0 mL of 0.1000 M NaOH. The excess NaOH is titrated with 20.00 mL of 0.2000 M HCl. Find the mass % of benzoic acid.
State whether each of the following substances is likely to be very soluble in water. Explain.
(a) Lithium nitrate
(b) Glycine
(c) Pentane
(d) Ethylene glycol
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