1. If MgBr2 forms the species Mg2+, Br-, MgBr+, and MgOH+ when placed in an aqueous...
1. If MgBr2 forms the species Mg2+, Br-, MgBr+, and MgOH+ when placed in an aqueous solution, what is the charge balance equation?
2. Calcium Phosphate, Ca3(PO4)2, is slightly soluble in water. Write the mass balance equation for an aqueous solution of calcium phosphate that forms calcium and phosphate ions when dissolved.
Homework Answers
1. Charge balance equation when MgBr2 is placed in aqueous solution ;
Total +ve charge species = total - ve charge species
2[Mg^+2]+[MgOH^+] + [H^+] + [MgBr^+] = [Br^-] + [OH^-]
Add Answer to:
1. If MgBr2 forms the species Mg2+,
Br-, MgBr+, and MgOH+ when placed
in an aqueous...
please explain. thanks 1. (a) 0.05 mole of MgBr2 is dissolved in 1 liter of solution...
please explain. thanks
1. (a) 0.05 mole of MgBr2 is dissolved in 1 liter of solution and the following species form: Mg2+, Br and MgOH' (a soluble hydroxy complex of Mg?) write a mass balance on the Mg species. Write a mass balance relating the molar concentration of Br to that of Mg species (b) write a charge balance for the solution in Part a.
L.2 yhen dissolved in water and neutralized with NH, AgCI forms the following species 1.2 r 4 (o)...
please answer question 6 & 7 and explain
not equation given
L.2 yhen dissolved in water and neutralized with NH, AgCI forms the following species 1.2 r 4 (o) (ay) 2(04) Mag) Write the charge balance for the equilibrium. [5) a. hat b. Write the mass balance for the reaction in silver (ie. lAgamobed).15 7. Beginning with the phosphate anion, show the stepwise process by which one obtains HsPO, in aqueous solution. Label equilibrium constants. [10 -o -at the near...
1. How many moles of ions are in the following solutions: 32.5mg potassium sulfate in water;...
1. How many moles of ions are in the following solutions: 32.5mg potassium sulfate in water; 1 mol MgBr2 in C6H6? 2. Given the following reaction and solubility data, how many moles of total ions are in solution once the reaction is complete starting with 25g of each reactant in 1L? Na3PO4 + Ca(NO3)2 --> NaNO3 + Ca3(PO4)2 COMPOUND SOLUBILITY SODIUM PHOSPHATE 94.6g/100mL CALCIUM NITRATE 120g/100mL SODIUM NITRATE 91.2g/100 mL CALCIUM PHOSPHATE 2mg/100mL
Identify the spectator ions present (if any) when aqueous solutions of AgNO3 and MgCl, are mixed....
Identify the spectator ions present (if any) when aqueous solutions of AgNO3 and MgCl, are mixed. Periodic Table TABLE 8.1 Solubility Rules for Ionic Compounds in Water Compounds Containing the Following Ions Are Generally Soluble Exceptions Lit, Nat, Kt, and NHA None NO, and C2H30 None CI, Br, and When these ions pair with Agt, Hg2+, or Pb2+, the resulting compounds are insoluble. SO2- When SO 2 pairs with Sr?+, Ba²+, Pb2+, Ag+, or Ca't, the resulting compound is insoluble....
1. Aqueous solutions should be electrically neutral. In other words, cations and anions should be balanced...
1. Aqueous solutions should be electrically neutral. In other words, cations and anions should be balanced with each other (charge balance) The following table shows the composition of typical seawater. 1. Set up a charge balance equation for the seawater. (b) Analyze the seawater whether is neutral or not. Note that the seawater constituent are expressed in mass concentrations. Constituent mg/kg (ppm) Sodium (Na*) 10,500 1,350 400 380 Magnesium (Mg2) Calcium (Ca2") Potassium (K) Chloride (Cl) Sulfate (SO2) Bicarbonate (HCO3)...
8. Solid Mg(OH)2 dissociates in water as shown below. The chemical equation for the autoprotolysis of...
8. Solid Mg(OH)2 dissociates in water as shown below. The chemical equation for the autoprotolysis of water is also shown. M8OH (aq) + OH"(aq) Mg(OH)2(s) MgOH (aq) Mg2*(aq) + OH (aq) OR Mg(OH)2(s) Mg2*(aq) +20H (aq) H2O*(aq) + OH (aq) 2H20( The middle equation can be represented in either of the two ways shown since the product ions are the same in both cases. For this solution, (A) write the correct charge-balance equation. [5 points] (B) write the correct mass-balance...
1. Predict the precipitate that forms when aqueous solutions of barium chloride and potassium sulfate are...
1. Predict the precipitate that forms when aqueous solutions of barium chloride and potassium sulfate are mixed? Write the overall and net ionic equation. Identify the spectator ions. 2. Write the balanced equation and the net ionic equation for the reaction of aluminum with hydrobromic acid? Determine which species is oxidized and which is reduced, as well as the oxidizing and reducing agents.
Complete and balance the following methesis reaction in aqueous solution. Instructions • Use proper element capitalization....
Complete and balance the following methesis reaction in aqueous solution. Instructions • Use proper element capitalization. Iron = Fe not fe. • Enter formulas without subscrips: CaCl2 = CaCl2, K2SO4 = K2SO4 • Monoatomic ions do not require parentheses. Correct: Na2CO3. Incorrect: (Na)2CO3 •Polyatomic ions only require parentheses when there are two or more. Correct: Na3PO4. Incorrect: Na3(PO4), Correct: NH4NO3. Incorrect: (NH4)(NO3). correct: Ca3(PO4)2 • In each case one product is soluble (aq) and one insoluble (s). Use solubility rules...
41 A solution is made 0.10 molar in Mo2+, 0.10 molar in NH3, and 1.0 molar...
41 A solution is made 0.10 molar in Mo2+, 0.10 molar in NH3, and 1.0 molar in NH,CI. ill Mg(OH)2 precipitate? 42 How many grams of ammonium chloride must be added to 100 ml of 0.050-molar ammonium hydroxide to revent the precipitation of ferrous hydroxide, Fe(OH)2, when the NH4CI- NH4OH mixture is added to 100 ml of 0.020-molar FeCl2? Assume that the addition of solid NH4Cl produces no volume change 43 The Ksp of calcium phosphate, Ca3(PO4)2, is 1.3 X...
1. Find all the pairs of ions in the following list which cannot exist together (in...
1. Find all the pairs of ions in the following list which cannot exist together (in appreciable concentration) in the same aqueous solution without precipitating. That is, write any combination of the following ions which would form a precipitate, a weak acid, a weak base, or water. [Note: PbCl2 is slightly soluble.] Fe3+ ht OH Na* ci" Pb2+ NO3 Mg2+ Answer: 2. Convert the following (a) complete or "molecular" equation to (b) the total ionic, and then to (c) the...
please explain. thanks
1. (a) 0.05 mole of MgBr2 is dissolved in 1 liter of solution and the following species form: Mg2+, Br and MgOH' (a soluble hydroxy complex of Mg?) write a mass balance on the Mg species. Write a mass balance relating the molar concentration of Br to that of Mg species (b) write a charge balance for the solution in Part a.
please answer question 6 & 7 and explain
not equation given
L.2 yhen dissolved in water and neutralized with NH, AgCI forms the following species 1.2 r 4 (o) (ay) 2(04) Mag) Write the charge balance for the equilibrium. [5) a. hat b. Write the mass balance for the reaction in silver (ie. lAgamobed).15 7. Beginning with the phosphate anion, show the stepwise process by which one obtains HsPO, in aqueous solution. Label equilibrium constants. [10 -o -at the near...
Identify the spectator ions present (if any) when aqueous solutions of AgNO3 and MgCl, are mixed. Periodic Table TABLE 8.1 Solubility Rules for Ionic Compounds in Water Compounds Containing the Following Ions Are Generally Soluble Exceptions Lit, Nat, Kt, and NHA None NO, and C2H30 None CI, Br, and When these ions pair with Agt, Hg2+, or Pb2+, the resulting compounds are insoluble. SO2- When SO 2 pairs with Sr?+, Ba²+, Pb2+, Ag+, or Ca't, the resulting compound is insoluble....
1. Aqueous solutions should be electrically neutral. In other words, cations and anions should be balanced with each other (charge balance) The following table shows the composition of typical seawater. 1. Set up a charge balance equation for the seawater. (b) Analyze the seawater whether is neutral or not. Note that the seawater constituent are expressed in mass concentrations. Constituent mg/kg (ppm) Sodium (Na*) 10,500 1,350 400 380 Magnesium (Mg2) Calcium (Ca2") Potassium (K) Chloride (Cl) Sulfate (SO2) Bicarbonate (HCO3)...
8. Solid Mg(OH)2 dissociates in water as shown below. The chemical equation for the autoprotolysis of water is also shown. M8OH (aq) + OH"(aq) Mg(OH)2(s) MgOH (aq) Mg2*(aq) + OH (aq) OR Mg(OH)2(s) Mg2*(aq) +20H (aq) H2O*(aq) + OH (aq) 2H20( The middle equation can be represented in either of the two ways shown since the product ions are the same in both cases. For this solution, (A) write the correct charge-balance equation. [5 points] (B) write the correct mass-balance...
41 A solution is made 0.10 molar in Mo2+, 0.10 molar in NH3, and 1.0 molar in NH,CI. ill Mg(OH)2 precipitate? 42 How many grams of ammonium chloride must be added to 100 ml of 0.050-molar ammonium hydroxide to revent the precipitation of ferrous hydroxide, Fe(OH)2, when the NH4CI- NH4OH mixture is added to 100 ml of 0.020-molar FeCl2? Assume that the addition of solid NH4Cl produces no volume change 43 The Ksp of calcium phosphate, Ca3(PO4)2, is 1.3 X...
1. Find all the pairs of ions in the following list which cannot exist together (in appreciable concentration) in the same aqueous solution without precipitating. That is, write any combination of the following ions which would form a precipitate, a weak acid, a weak base, or water. [Note: PbCl2 is slightly soluble.] Fe3+ ht OH Na* ci" Pb2+ NO3 Mg2+ Answer: 2. Convert the following (a) complete or "molecular" equation to (b) the total ionic, and then to (c) the...
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