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QUESTION 3 A soluble ionic species, SX, is dissolved in water. An excess of slightly soluble...
Solid Fe(OH)2 is slightly soluble in water. The Ksp = 1.6 x 10-14. What is the...
Solid Fe(OH)2 is slightly soluble in water. The Ksp = 1.6 x 10-14. What is the pH of a solution made from 0.2 mole of Fe(OH)2 (s) added added to 1.0 L solution of 0.039 M Fe(NO3)2(aq)? Note this is a review from chapter 15. There will be a problem like this on the exam. (A) 7.51 (B) 7.36 (C) 4.50 o (D) 7.81 (E) 4.99 Submit
QuesLIVIT 211.JPUITLS) The beaker below represents a solid ionic compound that has been dissolved in water...
QuesLIVIT 211.JPUITLS) The beaker below represents a solid ionic compound that has been dissolved in water to produce an aqueous solution. Based on the ratio of ions (assume one color is a cation and the other an anion), select all compounds below that could possibly represent the compound in the beaker below. Al2(SO4)3 Naci CaCl2 Na3PO4 Fe2(SO4)3 Na2CO3
Solid silver bromide (AgBr) will disassociate slightly in water to produce Agand Br". AgBr(s) + Agfaq) + Brīaq) Ksp = 1...
Solid silver bromide (AgBr) will disassociate slightly in water to produce Agand Br". AgBr(s) + Agfaq) + Brīaq) Ksp = 1.3 x 10-5 a. Calculate the equilibrium concentration of Ag+ if the solution if the solid AgBr is dissolved in pure water. Assume that the solution is behaving ideally (y = 1) b. Now let's explore the reaction if we take into account non-ideal behavior. Calculate the concentration of Ag+ in solution if the solid if the AgBr is dissolved...
b. MgCl, is dissolved in distilled water at 25°C until the saturated solution is obtained (system...
b. MgCl, is dissolved in distilled water at 25°C until the saturated solution is obtained (system reaches equilibrium). The concentration of Mg2 in the saturated solution is 1.35 x 10-'M. The dissolution of MgCl, in distilled water is endothermic. Write the balanced chemical equation to obtain the saturated solution Calculate the solubility product, K of MgCl2. Explain the effect of increasing the temperature on the amount of MgCl, Justify your answer. C. When solid Pbl, is added to pure water...
Part B please. Part A Silver chloride is only slightly soluble in pure water at 25...
Part B please.
Part A Silver chloride is only slightly soluble in pure water at 25 C AgCI(s) Ag (ag)+CI (aq) K-1.8 x 10 1 Calculate the concentration of Ag and Cl in a solution that is saturated with AgCl e, the system is at equilibrium and there is still solid AgCl visible). Express your answers using two significant figures, separate your answers by a comma. [Ag+],[Cl-)- 1.3×10-5 1.3×10-5 mol Li Previous An Correct Part B The addition of ammonia...
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...
Iodine is sparingly soluble in pure water. However, it does 'dissolve' in solutions containing excess iodide...
Iodine is sparingly soluble in pure water. However, it does 'dissolve' in solutions containing excess iodide ion because of the following reaction: 1(aq) + 12(aq) = 13(aq) K = 710. For each of the following cases calculate the equilibrium ratio of [13] to [12]. 5.00x10-2 mol of I2 is added to 1.00 L of 5.00x10-1 M KI solution. 3.20x102 You are correct. Previous Tries The solution above is diluted to 12.50 L. 7.09 Submit Answer You have entered that answer...
Calcium sulfate is only sparingly soluble. CaSO4(s) ⇌ Ca2+(aq) + SO42-(aq) For this type of dissolution...
Calcium sulfate is only sparingly soluble. CaSO4(s) ⇌ Ca2+(aq) + SO42-(aq) For this type of dissolution reaction the equilibrium constant, also known as the solubility product, is denoted Ks. In the reaction above, Ks = 8.8 x 10-6. When an excess of the solid is dissolved in water what is the maximum concentration of Ca2+(aq) in mol L-1? (Give your answer to at least TWO significant figures and do not include the units in the answer box. Hint: to help...
QUESTION 24 Which is a net ionic equation for the neutralization of a strong acid with...
QUESTION 24 Which is a net ionic equation for the neutralization of a strong acid with a strong base? HCl(aq) + NH3(aq) + NH4(aq) + Cl(aq) OB.H30(aq) + OH(aq) + 2 H2O() HF(aq) + NaOH(aq) = H2O()) + NaF(aq) OD. HF(aq) + OH-(aq) = H2000) + F(aq) QUESTION 25 Which of the following Bronsted-Lowry acids behaves as a strong acid when it is dissolved in water? O A HNO2 B. H3PO4 OC.H2504 OD.H2CO3 QUESTION 26 Which one of the following...
4.30. Using solubility rules, predict the solubility in water of the following ionic compounds. a. AI(OH) b. CaN...
4.30. Using solubility rules, predict the solubility in water of the following ionic compounds. a. AI(OH) b. CaN C. NH4CI d. KOH 4.32. Using solubility rules, decide whether the following ionic solids are soluble or insoluble in water. If they are soluble, write the chemical equation for dissolving in water and indicate what ions you would expect to be present in solution. (NE SO b. BaCO c. Pb(NOs)2 d. Ca(OH) 4.34. Write net ionic equations for the following molecular equations....
Solid Fe(OH)2 is slightly soluble in water. The Ksp = 1.6 x 10-14. What is the pH of a solution made from 0.2 mole of Fe(OH)2 (s) added added to 1.0 L solution of 0.039 M Fe(NO3)2(aq)? Note this is a review from chapter 15. There will be a problem like this on the exam. (A) 7.51 (B) 7.36 (C) 4.50 o (D) 7.81 (E) 4.99 Submit
QuesLIVIT 211.JPUITLS) The beaker below represents a solid ionic compound that has been dissolved in water to produce an aqueous solution. Based on the ratio of ions (assume one color is a cation and the other an anion), select all compounds below that could possibly represent the compound in the beaker below. Al2(SO4)3 Naci CaCl2 Na3PO4 Fe2(SO4)3 Na2CO3
Solid silver bromide (AgBr) will disassociate slightly in water to produce Agand Br". AgBr(s) + Agfaq) + Brīaq) Ksp = 1.3 x 10-5 a. Calculate the equilibrium concentration of Ag+ if the solution if the solid AgBr is dissolved in pure water. Assume that the solution is behaving ideally (y = 1) b. Now let's explore the reaction if we take into account non-ideal behavior. Calculate the concentration of Ag+ in solution if the solid if the AgBr is dissolved...
b. MgCl, is dissolved in distilled water at 25°C until the saturated solution is obtained (system reaches equilibrium). The concentration of Mg2 in the saturated solution is 1.35 x 10-'M. The dissolution of MgCl, in distilled water is endothermic. Write the balanced chemical equation to obtain the saturated solution Calculate the solubility product, K of MgCl2. Explain the effect of increasing the temperature on the amount of MgCl, Justify your answer. C. When solid Pbl, is added to pure water...
Part B please.
Part A Silver chloride is only slightly soluble in pure water at 25 C AgCI(s) Ag (ag)+CI (aq) K-1.8 x 10 1 Calculate the concentration of Ag and Cl in a solution that is saturated with AgCl e, the system is at equilibrium and there is still solid AgCl visible). Express your answers using two significant figures, separate your answers by a comma. [Ag+],[Cl-)- 1.3×10-5 1.3×10-5 mol Li Previous An Correct Part B The addition of ammonia...
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...
Iodine is sparingly soluble in pure water. However, it does 'dissolve' in solutions containing excess iodide ion because of the following reaction: 1(aq) + 12(aq) = 13(aq) K = 710. For each of the following cases calculate the equilibrium ratio of [13] to [12]. 5.00x10-2 mol of I2 is added to 1.00 L of 5.00x10-1 M KI solution. 3.20x102 You are correct. Previous Tries The solution above is diluted to 12.50 L. 7.09 Submit Answer You have entered that answer...
QUESTION 24 Which is a net ionic equation for the neutralization of a strong acid with a strong base? HCl(aq) + NH3(aq) + NH4(aq) + Cl(aq) OB.H30(aq) + OH(aq) + 2 H2O() HF(aq) + NaOH(aq) = H2O()) + NaF(aq) OD. HF(aq) + OH-(aq) = H2000) + F(aq) QUESTION 25 Which of the following Bronsted-Lowry acids behaves as a strong acid when it is dissolved in water? O A HNO2 B. H3PO4 OC.H2504 OD.H2CO3 QUESTION 26 Which one of the following...
4.30. Using solubility rules, predict the solubility in water of the following ionic compounds. a. AI(OH) b. CaN C. NH4CI d. KOH 4.32. Using solubility rules, decide whether the following ionic solids are soluble or insoluble in water. If they are soluble, write the chemical equation for dissolving in water and indicate what ions you would expect to be present in solution. (NE SO b. BaCO c. Pb(NOs)2 d. Ca(OH) 4.34. Write net ionic equations for the following molecular equations....
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