Concept explainers
Interpretation:
Whether
Concept introduction:
Solubility product in acid is equilibrium constant for reaction that occurs in acid solution when an ionic compound is dissolved to produce ions. It is represented by
The expression for its
A precipitate of an ionic compound will form when solutions that contain respective ions are mixed. The precipitation depends on value of reaction quotient
The expression for
Metal cations can be separated into two groups by the precipitation of metal sulfide. The cations which form very insoluble sulfides can be separated from cations which form soluble sulfides. The separation takes place in an acidic solution and use solubility equilibrium.
The separation depends on the
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CHEMISTRY-TEXT
- Which compound in each pair is more soluble in water than is predicted by a calculation from Ksp? (a) AgI or Ag2CO3 (b) PbCO3 or PbCl2 (c) AgCl or AgCNarrow_forwardFor each of the following insoluble salts, (1) write a balanced equation showing the equilibrium occurring when the salt is added to water, and (2) write the Ksp expression. (a) AgCN (b) NiCO3 (c) AuBr3arrow_forwardA solution is made up by adding 0.632 g of barium nitrate and 0.920 g of lanthanum nitrate, to La(NO3)3 enough water to make 0.500 L of solution. Solid sodium iodate, NalO3, is added (without volume change) to the solution. (a) Which salt will precipitate first? La(IO3)3 (Ksp=7.501012) or BAIO3 (Ksp=4.0109)? (b) What is [IO3-] when the salt in (a) first begins to precipitate?arrow_forward
- How do the concentrations of Ag+ and CrO42- in a saturated solution above 1.0 g of solid Ag2CrO4 Change when 100 g of solid Ag2CrO4 is added to the system? Explain.arrow_forwardA solution is 0.047 M in both NaF and Na2CO3. Solid strontium nitrate, Sr(NO3)2, is added without changing the volume of the solution. (a) Which salt, SrCO3 or SrF2(Ksp=4.3109), will precipitate first? (b) What is [Sr2+] when the salt in (a) first begins to precipitate?arrow_forwardWrite the Ksp expression for each of these slightly soluble salts: CuBr HgI2 SrSO4arrow_forward
- Write the ionic equation for the dissolution and the Ksp expression for each of the following slightly soluble ionic compounds: (a) LaF3. (b) CaCO3. (c) Ag2SO4. (d) Pb(OH)2arrow_forwardA buffer is made up of 0.300 L each of 0.500 M KH2PO4 and 0.317 M K2HPO4. Assuming that volumes are additive, calculate (a) the pH of the buffer. (b) the pH of the buffer after the addition of 0.0500 mol of HCl to 0.600 L of buffer. (c) the pH of the buffer after the addition of 0.0500 mol of NaOH to 0.600 L of buffer.arrow_forwardMarble is almost pure CaCO3. Acid rain has a devastating effect on marble statuary left outdoors. Assume that the reaction which occurs is CoCO3(s)+ H+(aq)Ca2+(aq)+HCO3(aq) Neglecting all other competing equilibria and using Tables 15.1 and 13.2, calculate (a) K for the reaction. (b) the molar solubility of CaCO3 in pure water. (c) the molar solubility of CaCO3 in acid rainwater with a pH of 4.00.arrow_forward
- For the titration of 50. mL of 0.10 M ammonia with 0.10 M HCI, calculate the pH. For ammonia, NH3, Kp = 1.8 x 10-5. (a) Before the addition of any HCl solution. pH = Use correct number of significant digits; (b) After 20. mL of the acid has been added. pH = Use correct number of significant digits; (c) After half of the NH3 has been neutralized. pH Use correct number of significant digits; (d) At the equivalence point. pH Use correct number of significant digits;arrow_forwardA solution contains 1.0 × 10–5 mol of KBr and 0.10 mol of KCl per liter. AgNO3 is gradually added to this solution. Which forms first, solid AgBr or solid AgCl?arrow_forwardA solution potentially contains Ag +, Ca2+, and Zn 2+ ions.First, HCl is added and a white precipitate forms. Thesolid is filtered out, then H 2 SO 4 is added and nothinghappens. Then H 2S is added and a black precipitate forms.Which cations are present? Which precipitates form?arrow_forward
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