Ion exchange reactions
1. Reactions of ion exchange include a reaction, the equation of which:
1) SO2 + 2NaOH \u003d Na2SO3 + H2O; 3) Na2SO3 + 2HCl \u003d 2NaCl + H2O + SO2;
2) Na2O + SO2 \u003d Na2SO3; 4) 2HCl + Zn \u003d ZnCl2 + H2.
2. The reaction of ion exchange corresponds to the equation:
1) Ca + 2H2O \u003d Ca (OH) 2 + H2; 3) 3H2O + P2O5 \u003d 2H3PO4;
2) Na2CO3 + 2HCl \u003d 2NaCl + H2O + CO2; 4) Na2O + SO2 \u003d Na2SO3.
3. Barium hydroxide solution enters into an ion exchange reaction:
1) with calcium sulfate solution; 3) with sodium chloride solution;
2) with carbon monoxide (IV); 4) with calcium carbonate.
4. A solution of copper (II) sulfate enters into an ion exchange reaction:
1) with a solution of silver chloride; 3) with iron;
2) with a solution of lithium hydroxide; 4) with silicic acid.
5. Are the the following judgments about ion exchange reactions?
A. Reactions of ion exchange occur in electrolyte solutions.
B. Reactions of ion exchange are practically feasible if the result is the formation of nondissociating or slightly dissociating substances.
1) Only A is true; 2) only B is true; 3) both judgments are correct; 4) both judgments are wrong.
6. Irreversible chemical reaction occurs when draining solutions:
1) calcium chloride and magnesium nitrate; 3) potassium phosphate and sodium bromide;
2) aluminum nitrate and copper (II) sulfate; 4) copper (II) chloride and barium hydroxide.
7. An irreversible chemical reaction will occur when solutions of substances are drained, the formulas of which:
1) ZnSO4 and HCl; 2) NaOH and KCl; 3) CuSO4 and HCl; 4) HNO3 and Ca (OH) 2.
8. The reaction between potassium hydroxide and hydrochloric acid corresponds to the abbreviated ionic equation:
1) Ag + + Cl- \u003d AgCl; 3) H + + OH- \u003d H2O;
2) Cu2 + + 2OH- \u003d Cu (OH) 2; 4) 2H + + CO32- \u003d H2O + CO2.
9. The reaction between zinc hydroxide and sulfuric acid corresponds to the abbreviated ionic equation:
1) H + + OH- \u003d H2O; 3) Zn (OH) 2 + 2H + \u003d Zn2 + + 2H2O;
2) Zn2 + + SO42- \u003d ZnSO4; 4) 2H + + SO42- \u003d H2SO4.
10. According to the reaction equation
3Cu2 + + 2PO43- \u003d Cu3 (PO4) 2,
possible interaction between:
1) zinc phosphate and copper (II) nitrate; 3) phosphoric acid and copper (II) oxide;
2) copper (II) hydroxide and sodium phosphate; 4) copper (II) chloride and phosphoric acid.
11. Abbreviated ionic equation
Fe2 + + 2OH- \u003d Fe (OH) 2
corresponds to the interaction of substances, the formulas of which:
1) FeCl3 and Ba (OH) 2; 3) Fe (NO3) 3 and KOH;
2) Fe (NO3) 2 and Na2S; 4) FeSO4 and LiOH.
12. An insoluble salt is formed by the action of barium hydroxide on a solution61) of sodium sulfate; 3) lithium nitrate;
2) hydrogen chloride; 4) copper (II) chloride.
13. An insoluble base is formed by the interaction of a potassium hydroxide solution with a solution:
1) sodium phosphate; 3) nitric acid;
2) iron (II) nitrate 4) potassium carbonate.
14. Insoluble acid is formed when a sodium silicate solution interacts with a solution:
1) lithium chloride; 3) sulfuric acid;
2) lithium hydroxide; 4) zinc nitrate.
15. Gas is not formed during the interaction of solutions:
1) sodium sulfide and sulfuric acid; 3) ammonium sulfate and potassium hydroxide;
2) potassium sulfide and copper (II) chloride; 4) lithium carbonate and of hydrochloric acid.
16. The precipitate is formed when the potassium hydroxide solution interacts with the solution:
1) sodium chloride; 3) copper (II) chloride;
2) ammonium chloride; 4) barium chloride.
17. The essence of the ion exchange reaction between barium chloride and each of the substances: sulfuric acid, copper (II) sulfate, ammonium sulfate - can be expressed by an abbreviated ionic equation:
1) Ba2 + + SO42- \u003d BaSO4; 3) Al3 + + 3OH- \u003d Al (OH) 3;
2) Ba2 + + 2OH- \u003d Ba (OH) 2; 4) 2 H + + SO32- \u003d H2O + SO2.
18. The essence of the ion exchange reaction between phosphoric acid and lithium hydroxide, nitric acid and potassium hydroxide, sulfuric acid and potassium hydroxide can be expressed by the abbreviated ionic equation:
1) 3Ca2 + + 2PO43- \u003d Ca3 (PO4) 2; 3) K + + NO3- \u003d KNO3;
2) H + + OH- \u003d H2O; 4) 2 H + + SO42- \u003d H2SO4.
19. To carry out the transformation, according to the abbreviated ionic equation:
Ca2 + + CO32- \u003d CaCO3,
nessesary to use:
1) calcium hydroxide solution and carbon dioxide; 3) solutions of calcium nitrate and sodium carbonate;
2) solutions of calcium chloride and sodium nitrate; 4) calcium oxide and carbon monoxide (IV).
20. To carry out the transformation, according to the short ionic equation
Zn2 + + 2 OH- \u003d Zn (OH) 2,
nessesary to use:
1) a solution of zinc nitrate and copper (II) hydroxide; 3) zinc oxide and potassium hydroxide solution;
2) a solution of zinc sulfate and calcium hydroxide; 4) solutions of zinc sulfate and potassium hydroxide.
21. When the solutions of sodium carbonate and sulfuric acid are merged, ions participate in the reaction:
1) CO32- and SO42-; 3) Na + and H +;
2) H + and CO32-; 4) Na + CO32-.
22. With the formation of a gaseous substance, a reaction takes place between solutions of substances, the formulas of which:
1) Na2S and HNO3; 3) KCl and Ca (OH) 2;
2) H2SO4 and CaCl2; 4) Cu (NO3) 2 and ZnSO4.
23. Each of two substances interacts with sodium hydroxide:
1) copper (II) chloride and silicic acid; 3) potassium sulfate and hydrogen sulfide acid;
2) aluminum phosphate and barium nitrate; 4) calcium carbonate and hydrochloric acid.
24. Hydrochloric acid can be used to detect ions:
1) K +; 2) Al3 +; 3) Cu2 +; 4) Ag +.
25. Sodium hydroxide solution can be used to detect ions:
1) Ba2 +; 2) Pb2 +; 3) Cs +; 4) SO32-
26. Establish a correspondence between the names of the starting substances and the sign of the reaction between them.
Starting materials: Signs of the reaction
A) potassium sulfide and nitric acid; 1) gas evolution;
B) aluminum sulfate and sodium hydroxide (insufficient); 2) precipitation;
B) lithium hydroxide and phosphoric acid; 3) the formation of low-dissociating D) potassium carbonate and sulfuric acid; substances (water).
Answer.
A B C D
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Option 1 Option 2 Answers: 161. The ion exchange reaction between solutions of 1) sodium chloride and copper (II) nitrate 2) sulfuric acid and barium nitrate 3) potassium sulfate and sodium hydroxide 4) potassium nitrate and iron (III) sulfate 162 The reaction of ion exchange between solutions of 1) sodium nitrate and copper (II) sulfate 2) sulfuric acid and potassium nitrate 3) potassium sulfate and barium hydroxide 4) sodium chloride and iron (III) sulfate
Ion exchange reactions and conditions for their implementation Option 1 Option 2 Answers: 163. The ion exchange reaction between solutions of 1) zinc nitrate and potassium sulfate 2) phosphoric acid and sodium chloride 3) potassium hydroxide and barium nitrate 4) sodium carbonate and hydrochloric acid 164. The reaction of ion exchange between solutions of 1) aluminum sulfate and potassium nitrate 2) sulfuric acid and calcium carbonate 3) sodium hydroxide and barium chloride 4) sodium nitrate and hydrochloric acid
Ion exchange reactions and conditions for their implementation Option 1 Option 2 Answers: 165. The ion exchange reaction between solutions of 1) sodium nitrate and calcium chloride 2) potassium sulfate and sodium hydroxide 3) copper (II) sulfate and sodium hydroxide 4) hydrochloric acid and magnesium nitrate 166. The reaction of ion exchange between solutions of 1) sodium sulfide and hydrochloric acid 2) sodium carbonate and potassium hydroxide 3) sulfuric acid and copper (II) nitrate 4) phosphoric acid and sodium chloride
Ion exchange reactions and the conditions for their implementation Option 1 Option 2 Answers: 167. A gaseous substance is formed by the interaction of solutions 1) potassium sulfate and nitric acid 2) sodium carbonate and hydrochloric acid 3) sulfuric acid and sodium hydroxide 4) sodium sulfide and calcium nitrate 168 The reaction of ion exchange between solutions of 1) potassium chloride and sulfuric acid 2) silver nitrate and iron (III) chloride 3) hydrochloric acid and ammonium sulfate 4) potassium carbonate and sodium hydroxide
Ion exchange reactions and conditions for their implementation Option 1 Option 2 Answers: 169. The precipitate is not formed when mixing solutions 1) sodium hydroxide and iron (II) nitrate 2) potassium sulfate and sodium hydroxide 3) potassium silicate and hydrochloric acid 4) potassium carbonate and calcium chloride 170. No precipitate is formed when solutions are mixed 1) sodium chloride and copper (II) nitrate 2) potassium sulfate and barium hydroxide 3) magnesium carbonate and phosphoric acid 4) potassium phosphate and barium chloride
Ion exchange reactions and conditions for their implementation Option 1 Option 2 Answers: 171. A gaseous substance is formed by the interaction of solutions of 1) hydrochloric acid and barium hydroxide 2) zinc nitrate and sodium sulfate 3) potassium carbonate and sulfuric acid 4) sodium hydroxide and nitric acid 172 A gaseous substance is formed by the interaction of solutions of 1) sulfuric acid and barium chloride 2) sodium sulfite and hydrochloric acid 3) potassium phosphate and calcium hydroxide 4) sodium hydroxide and aluminum chloride
Ion exchange reactions and conditions for their implementation Option 1 Option 2 Answers: 173. When a solution of potassium carbonate is added to a solution of calcium nitrate 1) a precipitate is formed 2) a gas is released 3) a precipitate is precipitated and a gas is released 4) no visible changes occur 174. When the solution is added potassium sulfate to a solution of lead nitrate 1) precipitate 2) gas is released 3) precipitate is precipitated and gas is released 4) no visible changes occur
Ion exchange reactions and conditions for their implementation Option 1 Option 2 Answers: 175. Barium hydroxide enters into an ion exchange reaction with 1) calcium carbonate 2) potassium sulfate 3) sodium chloride 4) sodium hydroxide 176. Copper (II) sulfate reacts ionic exchange with 1) iron 2) silver 3) sodium chloride 4) sodium hydroxide
I. Write down the equations for the dissociation of acids, indicate the weak and strong acid, for the corresponding acid, write the expression for the dissociation constant: 1) HJ, H 2 SO 3; 2) H 2 SO 4, H 2 S; 3) HF, HNO 3; 4) HClO 4, H 2 CO 3; 5) HNO 2, HCl.
II. The value of the solubility product of a poorly soluble electrolyte is given: 1) PbCl 2 PR \u003d 1.710 -5; 2) PR Ag 2 SO 4 \u003d 710 -5; 3) PR Ag 2 CrO 4 \u003d 210 -7; 4) PR HgI 2 \u003d 10 -26; 5) PR Pb (OH) 2 \u003d 510 -16
Write down the expression for the product of the solubility of a given electrolyte and calculate the equilibrium concentration of each of its ions in a saturated solution (see example 1.1).
III. The ion exchange reaction proceeds according to the equation: 1) CH 3 COOH + KOH \u003d…; 2) MnS + HCl \u003d ...; 3) HNO 2 + NaOH \u003d ...; 4) NH 4 OH + HNO 3 \u003d ...; 5) CaCO 3 + HCl \u003d….
Write down the molecular and ion-molecular reaction equation. Explain the possibility of a spontaneous reaction in the forward direction, calculating the value of Kc for it, using expression (4.1) - see example 4.1.
Control test option.
I. Specify the electrolytes in solutions of which ionic equilibria are established: 1) CaCO 3 2) HCN3) HNO 3 4) NaOH
II. Indicate electrolytes, the addition of which causes a shift of heterogeneous ionic equilibrium in a saturated solution of Fe (OH) 2 to the left - in the direction of weakening the dissociation of Fe (OH) 2 (in the direction of decreasing its solubility): 1) FeSO 4 2) HNO 3 3) Na 2 S 4) Ba(OH) 2
III. How does the pH value of an Н 2 SO 3 solution change when a Na 2 SO 3 solution is added to it:
1) pH increases 2) pH decreases 3) pH does not change
IV. In a solution of ampholyte Cr (OH) 3, equilibria were established: 3- + 3H + Cr (OH) 3 + 3H 2 OCr 3+ + 3OH - + 3H 2 O. As a result of the binding of which ions formed during the dissociation of Cr (OH) 3 , it dissolves in alkali: 1) H + 2) OH - 3) Cr 3+
V. The concentration of Ag + ions in the solution is 310 -4 mol / l, the concentration of Br ions is 5 равна10 -2 mol / l. Will AgBr precipitate, if its solubility product PR \u003d 510 -13: 1) yes2) no
Vi. Hydrolysis reactions are: 1) Na 2 CO 3 + H 2 O = NaHCO 3 + NaOH 2) FeCl 2 + H 2 O = FeOHCl + HCl
3) HCl + NaOH \u003d NaCl + H 2 O 4) CuSO 4 + 2NaOH \u003d Cu (OH) 2 + Na 2 SO 4
Vii. The ionic-molecular reaction equation Na 2 S + 2HCl \u003d 2NaCl + H 2 S is written:
1) 2Na + + S 2- + 2HCl \u003d 2NaCl + H 2 S 2) S 2- + 2H + \u003d H 2 S
3) Na + + Cl - \u003d NaCl 4) Na 2 S + 2H + \u003d 2Na + + H 2 S
VIII. The ionic molecular equation H + + OH - \u003d H 2 O corresponds to the following molecular equation: 1) NaHCO 3 + NaOH \u003d Na 2 CO 3 + H 2 O2) H 2 S + 2KOH \u003d K 2 S + 2H 2 O
3) Cu (OH) 2 + H 2 SO 4 \u003d CuSO 4 + 2H 2 O 4) Ba (OH) 2 + 2HNO 3 \u003d Ba (NO 3 ) 2 + 2H 2 O
IX. The equilibrium constant of the reaction Kc NH 4 + + H 2 O \u003d NH 4 OH + H + is written as:
1) (NH 4 OH + H + ) / (NH 4 + + H 2 O) 2) NH 4 + / (NH 4 OHH + ) 3) ( NH 4 + + H 2 O) / (NH 4 OH + H + ) 4) NH 4 OH H + / NH 4 +
X. The equilibrium constant Kc of the reaction Cu 2+ + H 2 O \u003d CuOH + + H + is numerically equal to: 1) K CuOH + / K H 2 O 2) K H 2 O / K CuOH + 3) K H 2 O
Answers and comments.
I– 1.2 (see item 1.2); II– 1.4 (see item 3 regarding the influence of ions of the same name on the state of ionic equilibrium); III– 1 (see item 3; as a result of a shift of ionic equilibrium to the left there is a binding of H + ions, ie, a decrease in their concentration, which, in accordance with expression (1.4), causes an increase in pH); IV– 1 (see example 3.4); V– 1 (see item 3, example 3.4); VI– 1.2 (see the definition of hydrolysis in item 5); VII– 2 (see the definition of the strength of electrolytes in item 2 and the rules for compiling ion-molecular reactions in item 4); VIII– 4 (a source of free ions in the left side of the ion-molecular equation can only be strong electrolytes - see item 2); IX– 4 (Kc is equal to the product of equilibrium concentrations of products, referred to the product of equilibrium concentrations of reagents; the concentration of H 2 O due to its constancy is not included in the expression Kc); X - 2 (see expression 4.1).
