Solve the whole box pleaseHomework Answers
[OH-] = 3M ×(1ml/3ml) = 1 M
[Mn+] = 0.1M ×(2ml/3ml) = 0.0667M , here M = Mg, Cu, Fe, Zn
| MgCl2 | CuSO4 | Fe(NO3)3 | Zn(NO3)2 | |
| Q | 0.0667×(1)2 = 0.0667 > Ksp | 0.0667×(1)2 = 0.0667 > Ksp | 0.0667×(1)3= 0.0667 > Ksp | 0.0667×(1)2 > Ksp |
| Ppt | Mg(OH)2 | Cu(OH)2 | Fe(OH)3 | Zn(OH)2 |
| Eq. | Mg2+ + 2 OH- ---> Mg(OH)2(s) | Cu2+ +2OH- ---> Cu(OH)2(s) | Fe3+ + 3 OH- ---> Fe(OH)3(s) | Zn2+ + 2OH- ---> Zn(OH)2(s) |
| Color | white | blue or blue-green | Reddish brown | White |
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Solve the whole box please
MgCl 0.1 M CuSO 0.1 M Fe(NO) 0.1 M Zn(NO)i 0.1...
2NaOH (aq) + MgCl; (aq) + 2NaCl (aq) + Mg(OH)2 (s),- how much 0.1 M NaOH...
2NaOH (aq) + MgCl; (aq) + 2NaCl (aq) + Mg(OH)2 (s),- how much 0.1 M NaOH solution will completely precipitate the Mg²+ in 0.8 L of 0.10 M MgCl, solution? Round to 2 significant figures. Provide your answer below: LNaOH FEEDBAC
Please show work for thumbs up! 6) A solution contains equal concentrations of Cu?", Co?, Fe?',...
Please show work for thumbs up!
6) A solution contains equal concentrations of Cu?", Co?, Fe?', and Mg". If we add 0.050 M sodium hydroxide (NaOH) to this solution dropwise, which ion will precipitate LAST? Compound K Cu(OH) 2.2 x 10 CO(OH), 5.92 x 10- Fe(OH) 4.87 x 10- Mg(OH) 2.06 x 10 b) A solution contains equal e sodium hydroxide (NaOH) to Compound Kop Cu(OH) 2.2 x 10-20 CO(OH)2 5.92 x 10-15 Fe(OH), 4.87 x 10-" Mg(OH) 2.06 x...
*redox reactions in electeochemical cells* c) Fe/0.1 M FeSO4//0.1 M CuSO4/Cu I soaked a porous cup in tap water for a few minutes and then i let it stand in a 100 ml beaker containing 10ml of 0.1 M Fe...
*redox reactions in electeochemical cells*
c) Fe/0.1 M FeSO4//0.1 M CuSO4/Cu
I soaked a porous cup in tap water for a few minutes and then i
let it stand in a 100 ml beaker containing 10ml of 0.1 M FeSO4. I
added enough 0.1M CuSO4 to the cup until the two liquid levels were
the same height. I inserted a zinc strip into the 0.1 M FeSO4 and a
shiny copper strip into the 0.1 M CuSO4. I connected the...
QUESTION 13 When 2 mL of 0.1 M aqueous HCI (hydrochloric acid) are added to a...
QUESTION 13 When 2 mL of 0.1 M aqueous HCI (hydrochloric acid) are added to a small strip of magnesium (Mg) what happens? A violent explosion O Nothing Bubbles of hydrogen are produced and the magnesium dissolves O The magnesium turns red and the solution goes yellow QUESTION 14 1 poi Which is the balanced chemical equation describing the reaction of question 13? O Mg(aq) + HCl(aq) → MgCl(s) + H(g) O Mg(s) + HCl(aq) - MgCl (aq) + H2(g)....
1.2 Mg + 1 ou 2 Mgo 2. 2 A1+_LN AIN 33 Fe + 20,- |...
1.2 Mg + 1 ou 2 Mgo 2. 2 A1+_LN AIN 33 Fe + 20,- | Fe:0. H₂O + 0₂ 2H₂O2-2 H 2042 NH.NO, N,0 +_ _H20 AgNO3 +_ _Zn → __Zn(NO3)2 + Ag Na +_ H2O + NaOH + H2 Fe(OH)3 + __H2SO4 → ___ Fe(SO.)3 + ___ H20 AgNO3 + __ H2S → __ AgzS + __HNO, Al +_ Fe,Og → Fe +_ _A1,03 Cu + __ Ag,SO. → __ Cuso, + __ Ag NH, + O +...
Partner's Name Instructor Procedure I, Voltaic Cell Zn/Zn2+ 1.0 M || Cu2+ 1.0 M/Cu In the...
Partner's Name Instructor Procedure I, Voltaic Cell Zn/Zn2+ 1.0 M || Cu2+ 1.0 M/Cu In the space below write the equations for the two half reactions and sum them appropriately to calculate the standard reaction potential for a 1.0 M voltaic cell. Show the overall net ionic equation for this reaction. 9pts.) Standard reaction potential Write the expression for Q for this redox reaction. (4 pes) In the space below show a calculation using the Nemst equation to determine the...
4) (24 points) What is the solubility of Fe(OH)s (iron(III) hydroxide)... a) ...pure water? b) ...0.036...
4) (24 points) What is the solubility of Fe(OH)s (iron(III) hydroxide)... a) ...pure water? b) ...0.036 M Fe(NO3)3? Ka values: HCI HNO3 H2SO4 HSOF 113x102 HsPO7.5 x 103 HF HNO2 strong CH3COOH 1.8 x 10 CHNHF 5.9 x 106 HCO 4.2x 10 H2CO3 strong HaPO 62x 10 H2PO4 7.1 x 104 4.5 x 1 HCN HCO3 HPO4 4.9 x 10 48 x 101 1.7 x 10" HCOOH Ksp values: Mg(OH)212x 10 | AgBr _ 17,7 x10.TS- і I 8.7 x...
3. Suppose after adding HCl to ppt 16, you do not have any black solid. What,...
3. Suppose after adding HCl to ppt 16, you do not have any black solid. What, if anything, should you do to test for Co2 and Ni*? Qual Scheme: Group III: Co?(pink), N1" (green), Fet+ (yellow), Cr" (blue-grey), Mn(pink), AP (colorless), Zn? (colorless). Unknown B Solution: Use 10 dps of unknown sample and 10 dps of H20 and go to Procedure for Group III. Procedure for Group II: Add 2 dps NHCl soln, add 6M NHOH until just basic to...
please box answers and in understandable handwritng thanks O Even to Last Response 2. -/0.1 points...
please box answers and in understandable handwritng thanks
O Even to Last Response 2. -/0.1 points 0/4 Submissions Used Assume you dissolve 0.235 g of the weak acid benzoic acid, C.HCO2H, in enough water to make 7.00 x 102mL of solution and then titrate the solution with 0.138 M NaOH. CHECO2H(aq) + OH(aq) + CHCO2 (aq) + H2010 What are the concentrations of the following ions at the equivalence point? Na*, H30, OH CH5CO2 M Na MHz0+ Мон" M CHECO2...
A solution contains equal concentrations of Ba2+, Ca", Mg?", and Zn". If we begin adding 0.1...
A solution contains equal concentrations of Ba2+, Ca", Mg?", and Zn". If we begin adding 0.1 M sodium oxalate (Na2C_04) to this solution dropwise, which ion will begin precipitating first? Compound Ksp BaC204 1.6 x 10 CaC204 2.32 x 10 MgC20 4.83 x 10 ZnC2042.7 x 108 Determine the pH required for the onset of the precipitation of Ni(OH)2 from a 0.010-M NISO.(ag) solution at 25° C. At 25°C, K for Ni(OH)2 is 6.5 x 10-18
2NaOH (aq) + MgCl; (aq) + 2NaCl (aq) + Mg(OH)2 (s),- how much 0.1 M NaOH solution will completely precipitate the Mg²+ in 0.8 L of 0.10 M MgCl, solution? Round to 2 significant figures. Provide your answer below: LNaOH FEEDBAC
Please show work for thumbs up!
6) A solution contains equal concentrations of Cu?", Co?, Fe?', and Mg". If we add 0.050 M sodium hydroxide (NaOH) to this solution dropwise, which ion will precipitate LAST? Compound K Cu(OH) 2.2 x 10 CO(OH), 5.92 x 10- Fe(OH) 4.87 x 10- Mg(OH) 2.06 x 10 b) A solution contains equal e sodium hydroxide (NaOH) to Compound Kop Cu(OH) 2.2 x 10-20 CO(OH)2 5.92 x 10-15 Fe(OH), 4.87 x 10-" Mg(OH) 2.06 x...
*redox reactions in electeochemical cells*
c) Fe/0.1 M FeSO4//0.1 M CuSO4/Cu
I soaked a porous cup in tap water for a few minutes and then i
let it stand in a 100 ml beaker containing 10ml of 0.1 M FeSO4. I
added enough 0.1M CuSO4 to the cup until the two liquid levels were
the same height. I inserted a zinc strip into the 0.1 M FeSO4 and a
shiny copper strip into the 0.1 M CuSO4. I connected the...
QUESTION 13 When 2 mL of 0.1 M aqueous HCI (hydrochloric acid) are added to a small strip of magnesium (Mg) what happens? A violent explosion O Nothing Bubbles of hydrogen are produced and the magnesium dissolves O The magnesium turns red and the solution goes yellow QUESTION 14 1 poi Which is the balanced chemical equation describing the reaction of question 13? O Mg(aq) + HCl(aq) → MgCl(s) + H(g) O Mg(s) + HCl(aq) - MgCl (aq) + H2(g)....
1.2 Mg + 1 ou 2 Mgo 2. 2 A1+_LN AIN 33 Fe + 20,- | Fe:0. H₂O + 0₂ 2H₂O2-2 H 2042 NH.NO, N,0 +_ _H20 AgNO3 +_ _Zn → __Zn(NO3)2 + Ag Na +_ H2O + NaOH + H2 Fe(OH)3 + __H2SO4 → ___ Fe(SO.)3 + ___ H20 AgNO3 + __ H2S → __ AgzS + __HNO, Al +_ Fe,Og → Fe +_ _A1,03 Cu + __ Ag,SO. → __ Cuso, + __ Ag NH, + O +...
Partner's Name Instructor Procedure I, Voltaic Cell Zn/Zn2+ 1.0 M || Cu2+ 1.0 M/Cu In the space below write the equations for the two half reactions and sum them appropriately to calculate the standard reaction potential for a 1.0 M voltaic cell. Show the overall net ionic equation for this reaction. 9pts.) Standard reaction potential Write the expression for Q for this redox reaction. (4 pes) In the space below show a calculation using the Nemst equation to determine the...
4) (24 points) What is the solubility of Fe(OH)s (iron(III) hydroxide)... a) ...pure water? b) ...0.036 M Fe(NO3)3? Ka values: HCI HNO3 H2SO4 HSOF 113x102 HsPO7.5 x 103 HF HNO2 strong CH3COOH 1.8 x 10 CHNHF 5.9 x 106 HCO 4.2x 10 H2CO3 strong HaPO 62x 10 H2PO4 7.1 x 104 4.5 x 1 HCN HCO3 HPO4 4.9 x 10 48 x 101 1.7 x 10" HCOOH Ksp values: Mg(OH)212x 10 | AgBr _ 17,7 x10.TS- і I 8.7 x...
3. Suppose after adding HCl to ppt 16, you do not have any black solid. What, if anything, should you do to test for Co2 and Ni*? Qual Scheme: Group III: Co?(pink), N1" (green), Fet+ (yellow), Cr" (blue-grey), Mn(pink), AP (colorless), Zn? (colorless). Unknown B Solution: Use 10 dps of unknown sample and 10 dps of H20 and go to Procedure for Group III. Procedure for Group II: Add 2 dps NHCl soln, add 6M NHOH until just basic to...
please box answers and in understandable handwritng thanks
O Even to Last Response 2. -/0.1 points 0/4 Submissions Used Assume you dissolve 0.235 g of the weak acid benzoic acid, C.HCO2H, in enough water to make 7.00 x 102mL of solution and then titrate the solution with 0.138 M NaOH. CHECO2H(aq) + OH(aq) + CHCO2 (aq) + H2010 What are the concentrations of the following ions at the equivalence point? Na*, H30, OH CH5CO2 M Na MHz0+ Мон" M CHECO2...
A solution contains equal concentrations of Ba2+, Ca", Mg?", and Zn". If we begin adding 0.1 M sodium oxalate (Na2C_04) to this solution dropwise, which ion will begin precipitating first? Compound Ksp BaC204 1.6 x 10 CaC204 2.32 x 10 MgC20 4.83 x 10 ZnC2042.7 x 108 Determine the pH required for the onset of the precipitation of Ni(OH)2 from a 0.010-M NISO.(ag) solution at 25° C. At 25°C, K for Ni(OH)2 is 6.5 x 10-18
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