(10 pts) The graph below shows solubility vs. pH for five solids (where solubility in M is the same as the dissolved metal cations). These solids are hydroxides of chromium (Cr), aluminum (Al), nickel (Ni), and iron (Fe in II and III oxidation states; often referred to as ferrous and ferric iron). Use this graph to answer parts a-c below.
- a) Which solid is among the least soluble at pH 12 and among the most soluble at pH 6?
- b) Over what pH range would it be possible to precipitate nickel hydroxide while leaving aluminum fully dissolved?
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(10 pts) The graph below shows solubility vs.
pH for five solids (where solubility in M...
Below is a Ksp Table of many common hydroxides used frequently in chemistry. If you were...
Below is a Ksp Table of many common hydroxides used frequently in chemistry. If you were given a set of ions to convert to hydroxides, which 2 ions would be the easiest to separate? a) Cobalt and Iron b) Magnesium and Calcium c) Nickel and iron d) Cobalt and Calcium e) Copper and Zinc Circle the above pair and explain your reasoning: Al(OH)3 Cd(OH) Ca(OH)2 Cr(OH)3 CO(OH) 3 Co(OH)2 Cu(OH) 2 Fe(OH), Fe(OH) 2 Pb(OH)2 Mg(OH)2 Mn(OH) 2 Ni(OH) 2...
48 Group III Cations Scheme Fo”, Ni, Cr", Alto 3% H2O2 (Step 3) 6M NaOH (Step...
48 Group III Cations Scheme Fo”, Ni, Cr", Alto 3% H2O2 (Step 3) 6M NaOH (Step 4) Heat (Step 5) Fe(OH). (brown solid) NI(OH) (green solid) (Black solid, Step 6) Croi (Al(OH) (Yellow solution, Step 6) 1 15M HNO, (Step 7) 1M NHACI (Step 8) 15M NH,OHNH, (Step 9)/Spin (Step 10) 15M HNO, (Step 14) GM NH,OHNH, (Step 15) Fe(OH) (Brown solid Step 10) INIINHA (Blue solution Step 10) Al(OH) White gel Step 16) Cro. (Yellow solution Step 16) 1...
An acidic solution is 2 mM in each of the following metal ions: Zn2+, Cu2+, Co2+,...
An acidic solution is 2 mM in each of the following metal ions: Zn2+, Cu2+, Co2+, Ca2+. a) Which of the metals would precipitate as their hydroxides at pH = 6.00? (Select all that apply. See theappendix.) -zinc -copper -cobalt -calcium b) Which of the metals would precipitate as their hydroxides at pH = 8.00? -zinc -copper -cobalt -calcium c) At what pH do the metal hydroxides begin to participate? Zn(OH)2 ____ Cu(OH)2 ____ Co(OH)2 ____ Ca(OH)2 ____ Substance Ksp...
1. Using Table 38.3 in the Voyce text, calculate the solubility of Manganese(II) hydroxide at 25oC...
1.
Using Table 38.3 in the Voyce text, calculate the solubility of
Manganese(II) hydroxide at 25oC
A.
5.7 x 10-5
B.
3.6 x 10-5
C.
4.4 x 10-7
2.
The pH of a 0.0147M KCN solution is:
A.
10.7
B.
5.52
C.
3.3
D.
8.48
3.
The pH of a buffer solution composed of 0.020M HCHO2
and 0.014M NaCHO2 is:
A.
3.59
B.
3.74
C.
3.90
4.
When 400ml of a 0.01M SnCl2 solution is mixed with a
300ml if...
need help, convert them like below pic S. OH- t. 10 w. CIO2 2- X. CO24...
need help, convert them like below pic
S. OH- t. 10 w. CIO2 2- X. CO24 y. HSO3 z. CIO, u. HCO3- v. 104 5. Ionic Compounds with Polyatomic lons & Constant Charge lons a. CaCO3 i. potassium hydroxide b. KCIO j. beryllium hydroxide C. CASO k. strontium acetate d. Li2SO3 I. ammonium oxide e. Ag3PO4 m. silver cyanide f. NH,F n. zinc carbonate g. Al(NO2)3 0. aluminum bicarbonate h. Ba(HCO3)2- p. magnesium phosphate b. NiP04 6. Tonic Compounds with...
a) 4.9 x 10'M b)24x10 M c)5.8x 1010 M )1.2 x 10 M 19. Which one of the following compounds will have the lowest molar solubility in pur water? b) CuS, Ksp 1.27x103 d) ZnS, Ksp = 1.6 x 10-24 a...
a) 4.9 x 10'M b)24x10 M c)5.8x 1010 M )1.2 x 10 M 19. Which one of the following compounds will have the lowest molar solubility in pur water? b) CuS, Ksp 1.27x103 d) ZnS, Ksp = 1.6 x 10-24 a) PbS, Ksp 9.04 x 102 e) Al(OH)s, Ksp 3 x 1034 What is the molar solubility, i.e. [Fe , in a saturated aqueous solution of 20. Fe(OH)20) Fe(OH(s)Fe2+(aa) + 201H (ag), Ksp 4.87 x 101" a) 2.44 x 1017...
1. A solution contains 8.68×10-3 M sodium hydroxide and 6.04×10-3 M ammonium sulfide. Solid manganese(II) nitrate...
1. A solution contains 8.68×10-3 M sodium hydroxide and 6.04×10-3 M ammonium sulfide. Solid manganese(II) nitrate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of manganese(II) ion when this precipitation first begins? [Mn2+] = M 2. A solution contains 5.04×10-3 M magnesium nitrate and 1.31×10-2 M nickel(II) acetate. Solid sodium hydroxide is added slowly to this mixture. A. What is the formula of...
Solubility Product Constants (Ksp at 25 °C) Type Formula Кsp Bromides PbBr2 6.3 x 10-6 AgBr...
Solubility Product Constants (Ksp at 25 °C) Type Formula Кsp Bromides PbBr2 6.3 x 10-6 AgBr 3.3 * 10-13 Carbonates BaCO3 8.1 x 10-9 CaCO3 3.8 x 10-9 COCO3 8.0 × 10-13 CuCO3 2.5 10-10 FeCO3 3.5 x 10-11 PbCO3 1.5 10-13 MgCO3 4.0 x 10-5 MnCO3 1.8 10-11 NiCO3 6.6 x 10-9 Ag2CO3 8.1 x 10-12 ZnCO3 1.5 x 10-11 Chlorides PbCl2 1.7 x 10-5 AgC1 1.8 10-10 Chromates BaCrO4 2.0 x 10-10 CaCrO4 7.1 x 10-4 PbCr04 1.8...
Consider the titration of a 40.0 ml. of 0.155 M weak acid HA (Ka = 2.7...
Consider the titration of a 40.0 ml. of 0.155 M weak acid HA (Ka = 2.7 x 10") with 0.100 M LiOH. What is the pH of the solution before any base has been added? L 4 points b What would be the pH of the solution after the addition of 200 ml of LiOH? 4 points How many mL of the LiOH would be required to reach the halfway point of the titration? 1 4 points points d What...
I need the answers for page 2 and three do not pay attention to the first...
I
need the answers for page 2 and three do not pay attention to the
first page!
EXPERIMENT 10: DETERMINATION OF THE ELECTROCHEMICAL SERIES QUESTIONS Which metal was not oxidized by any of the other half-cells? 1. Using Table 1, what are two metal half-cells that would oxidize the metal from question #1? 2 3. Which metal was oxidized by all of the other half-cells? 4. Using Table 1, what are two metal half-cells that the metal from question #3...
Below is a Ksp Table of many common hydroxides used frequently in chemistry. If you were given a set of ions to convert to hydroxides, which 2 ions would be the easiest to separate? a) Cobalt and Iron b) Magnesium and Calcium c) Nickel and iron d) Cobalt and Calcium e) Copper and Zinc Circle the above pair and explain your reasoning: Al(OH)3 Cd(OH) Ca(OH)2 Cr(OH)3 CO(OH) 3 Co(OH)2 Cu(OH) 2 Fe(OH), Fe(OH) 2 Pb(OH)2 Mg(OH)2 Mn(OH) 2 Ni(OH) 2...
48 Group III Cations Scheme Fo”, Ni, Cr", Alto 3% H2O2 (Step 3) 6M NaOH (Step 4) Heat (Step 5) Fe(OH). (brown solid) NI(OH) (green solid) (Black solid, Step 6) Croi (Al(OH) (Yellow solution, Step 6) 1 15M HNO, (Step 7) 1M NHACI (Step 8) 15M NH,OHNH, (Step 9)/Spin (Step 10) 15M HNO, (Step 14) GM NH,OHNH, (Step 15) Fe(OH) (Brown solid Step 10) INIINHA (Blue solution Step 10) Al(OH) White gel Step 16) Cro. (Yellow solution Step 16) 1...
1.
Using Table 38.3 in the Voyce text, calculate the solubility of
Manganese(II) hydroxide at 25oC
A.
5.7 x 10-5
B.
3.6 x 10-5
C.
4.4 x 10-7
2.
The pH of a 0.0147M KCN solution is:
A.
10.7
B.
5.52
C.
3.3
D.
8.48
3.
The pH of a buffer solution composed of 0.020M HCHO2
and 0.014M NaCHO2 is:
A.
3.59
B.
3.74
C.
3.90
4.
When 400ml of a 0.01M SnCl2 solution is mixed with a
300ml if...
need help, convert them like below pic
S. OH- t. 10 w. CIO2 2- X. CO24 y. HSO3 z. CIO, u. HCO3- v. 104 5. Ionic Compounds with Polyatomic lons & Constant Charge lons a. CaCO3 i. potassium hydroxide b. KCIO j. beryllium hydroxide C. CASO k. strontium acetate d. Li2SO3 I. ammonium oxide e. Ag3PO4 m. silver cyanide f. NH,F n. zinc carbonate g. Al(NO2)3 0. aluminum bicarbonate h. Ba(HCO3)2- p. magnesium phosphate b. NiP04 6. Tonic Compounds with...
a) 4.9 x 10'M b)24x10 M c)5.8x 1010 M )1.2 x 10 M 19. Which one of the following compounds will have the lowest molar solubility in pur water? b) CuS, Ksp 1.27x103 d) ZnS, Ksp = 1.6 x 10-24 a) PbS, Ksp 9.04 x 102 e) Al(OH)s, Ksp 3 x 1034 What is the molar solubility, i.e. [Fe , in a saturated aqueous solution of 20. Fe(OH)20) Fe(OH(s)Fe2+(aa) + 201H (ag), Ksp 4.87 x 101" a) 2.44 x 1017...
Solubility Product Constants (Ksp at 25 °C) Type Formula Кsp Bromides PbBr2 6.3 x 10-6 AgBr 3.3 * 10-13 Carbonates BaCO3 8.1 x 10-9 CaCO3 3.8 x 10-9 COCO3 8.0 × 10-13 CuCO3 2.5 10-10 FeCO3 3.5 x 10-11 PbCO3 1.5 10-13 MgCO3 4.0 x 10-5 MnCO3 1.8 10-11 NiCO3 6.6 x 10-9 Ag2CO3 8.1 x 10-12 ZnCO3 1.5 x 10-11 Chlorides PbCl2 1.7 x 10-5 AgC1 1.8 10-10 Chromates BaCrO4 2.0 x 10-10 CaCrO4 7.1 x 10-4 PbCr04 1.8...
Consider the titration of a 40.0 ml. of 0.155 M weak acid HA (Ka = 2.7 x 10") with 0.100 M LiOH. What is the pH of the solution before any base has been added? L 4 points b What would be the pH of the solution after the addition of 200 ml of LiOH? 4 points How many mL of the LiOH would be required to reach the halfway point of the titration? 1 4 points points d What...
I
need the answers for page 2 and three do not pay attention to the
first page!
EXPERIMENT 10: DETERMINATION OF THE ELECTROCHEMICAL SERIES QUESTIONS Which metal was not oxidized by any of the other half-cells? 1. Using Table 1, what are two metal half-cells that would oxidize the metal from question #1? 2 3. Which metal was oxidized by all of the other half-cells? 4. Using Table 1, what are two metal half-cells that the metal from question #3...
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