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(a)
Interpretation:
Concentration of
Concept Introduction:
The equilibrium constant used for the partially soluble salt in water is termed as solubility product constant
The expression for
Generally the concentration of solid is taken as constant. Therefore the expression for
(b)
Interpretation:
Mass of
Concept Introduction:
Concentration of solution is expressed in terms of molarity. It is the ratio of moles of solute to the volume of solution in litres. The expression used to determine the concentration of solution is as follows:
Mole is the unit that measures the quantity such as atoms, volume and molecules. It is the ratio of given mass to molecular mass of substance. It is expressed as follows:
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Chapter 16 Solutions
FOUND.OF COLLEGE CHEMISTRY
- Write the net ionic equation in which the slightly soluble salt barium fluoride, BaF2, dissolves in dilute hydrochloric acid.arrow_forwardWhat must be the concentration of chromate ion in order to precipitate strontium chromate, SrCrO4, from a solution that is 0.0034 M Sr2+?arrow_forwardA solution is 1.5 104 M Zn2 and 0.20 M HSO4. The solution also contains Na2SO4. What should be the minimum molarity of Na2SO4 to prevent the precipitation of zinc sulfide when the solution is saturated with hydrogen sulfide (0.10 M H2S)?arrow_forward
- Consider the reaction BaF2(s)+SO42(aq)BaSO4(s)+2 F(aq) (a) Calculate K for the reaction. (b) Will BaSO4 precipitate if Na2SO4 is added to a saturated solution of BaF2?arrow_forwardAcrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’. What is the pH of a 0.11 M solution of acrylic acid, CH2CHCOOH?arrow_forwardYou have 25.00 mL of a 0.100 M aqueous solution of the weak base (CH3)2NH (Kb = 7.40 x 10-4). This solution will be titrated with 0.100 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? ( c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution at the equivalence point of the titration? (e) What is the pH of the solution when 30.00 mL of acid has been added?arrow_forward
- For the titration of 25.00 mL of 0.100M CH CO,H with 0.100 M NAOH. The reaction can be represented as: CH,CO,H + OH- → CH,CO, + H,0 (a) What is the initial pH before any amount of the NaOH solution has been added?K: 1.8 x 10 for CH,CO,H. (b) Find the pH after 12.50 mL of the NaOH solution have been added. (c) Find the pH after 25.00 mL of the NAOH solution has been added. (d) Find the pH after 3750 mL of the NaOH solution has beern added.arrow_forwardPlease explain.arrow_forwardA buffer solution is made that is 0.307 M in HCN and 0.307 M in KCN. If K, for HCN is 4.00 × 10¬10, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.063 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) +arrow_forward
- 2arrow_forward(a) Lactic acid, (CH3CH(OH)COOH) is a common biomolecule which can accumulate in muscles during intense exercise. A chemist prepares a buffer using 225 mL of 85 M lactic acid (Ka = 1.38 x 10-4) and 435 mL of 0.68 M sodium lactate. What is the pH of the buffer? What is the pH of the lactate buffer if 0.25 moles of gaseous HCl is added?arrow_forwardA buffer solution contains 0.77 mol of hydrosulfuric acid (H2S) and 0.43 mol of sodium hydrogen sulfide (NaHS) in 5.70 L.The Ka of hydrosulfuric acid (H2S) is Ka = 9.5e-08.(a) What is the pH of this buffer?(b) What is the pH of the buffer after the addition of 0.44 mol of NaOH? (assume no volume change)(c) What is the pH of the original buffer after the addition of 0.08 mol of HI? (assume no volume change)arrow_forward
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