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What are the respective concentrations (M) of K and CO32- afforded by dissolving 0.530 mol K2CO3...
What are the respective concentrations (M) of Cu2+ and Cl- afforded by dissolving 0.833 mol CuCl2...
What are the respective concentrations (M) of Cu2+ and Cl- afforded by dissolving 0.833 mol CuCl2 in water and diluting to 375 mL? a. 0.00175 and 0.00175 b. 1.75 and 0.00175 c. 0.570 and 0.198 d. 0.00175 and 1.75 e. 1.75 and 3.51
Q29 What are the respective concentrations (M) of Cu^2+ and CI^- afforded by dissolving 0.741 mol...
Q29
What are the respective concentrations (M) of Cu^2+ and CI^- afforded by dissolving 0.741 mol CuCl_2 in water and diluting to 726mL? 0.00102 and 1.02 1.02 and 2.04 1.02 and 1.02 0.980 and 0.269 0.00102 and 0.00102
What are the respective concentrations ( M ) of Fe^3+ and 1 afforded by dissolving 0.200...
What are the respective concentrations ( M ) of Fe^3+ and 1 afforded by dissolving 0.200 moI Fel3 In 725 mL of water?
Calculate the pH of a solution that is prepared by dissolving 0.297 mol of pentafluorobenzoic acid...
Calculate the pH of a solution that is prepared by dissolving 0.297 mol of pentafluorobenzoic acid (CF.COOH, K, -3.30x10-2) and 0.650 mol of hydrocyanic acid (HCN, K, = 6.17x10-10) in water and diluting to 5.90 L. Also, calculate the equilibrium concentrations of C F COOH, C F C00", HCN, and CN. Do not make an approximation unless the initial acid concentration is greater than 1000 × K. (Hint: The pH will be determined by the stronger acid of this pair.)...
please help me please i dont have questions remaining anymore A solution is prepared by dissolving 0.060 mol of iodoacet...
please help me please i dont
have questions remaining anymore
A solution is prepared by dissolving 0.060 mol of iodoacetic acid (Kg = 6.68x10-4) and 0.040 mol of sodium iodoacetate in water to a total solution volume of 1.00 L. First, calculate a pH for the solution by assuming that the concentrations of ICH CO2H and ICH CO2 are equal to the formal concentrations of the substances dissolved. Submit Answer Tries 0/5 Next, calculate the pH for the solution based...
2. What is the pH of a solution which is 0.25 M KHCO, if the K,...
2. What is the pH of a solution which is 0.25 M KHCO, if the K, for HCOs is 2.4 x 10*2 Calculate the concentrations of НЗО", ОН, NHs, and cr in a solution prepared by dissolving 535 g of NH4CI in enough water to make 5.00 × 102 miL of solution at 25 °C., for NII is 1.8 x io-s. Hint: Is the given ionization constant for NHs the correct value to use in your calculations?) 3.
A solution is prepared by dissolving 0.23 mol of formic acid and 0.27 mol of sodium...
A solution is prepared by dissolving 0.23 mol of formic acid and 0.27 mol of sodium formate in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. The pH does not increase drastically because the NaOH reacts with the present in the buffer solution. The K, of formic acid is 1.8 x 10+ A formic acid B. sodium formate C water D. sodium E....
3.355 M K2SO4 solution can be prepared by A) dilution of 500.0 mL of 1.00 MK2SO4...
3.355 M K2SO4 solution can be prepared by A) dilution of 500.0 mL of 1.00 MK2SO4 to 1.00 L B) dissolving 46.7 g of K2SO4 in water and diluting to 500.0 ml, then diluting 25.0 ml of this solution to a total volume of 500.0 mL C) dissolving 46.7 g of K2SO4 in water and diluting to a total volume of 250.0 mL D) dilution of 1.00 mL of 0.355 M K2SO4 to 1.00 L E) diluting 46.7 mL of...
Bral -6.3 x 102 M & (Br)-1.2 x10 M. What are the equilibrium concentrations of Br,...
Bral -6.3 x 102 M & (Br)-1.2 x10 M. What are the equilibrium concentrations of Br, & Br at 1280C where K, 1.1 x 10'? Show ALL work (hint: test Q first) 9) Calculate (CoL,[Ch] & [COCk] when 5.00 mol COCI, decomposes&reaches equilibrium in 10.Ol flask. K 8.3 x 10* at 360°C 10) Reaction of 0.1050 mol PCl, w/0.0450 mol Cl, & 0.0450 mol PCl, in 0.5000 L flask. K, 4.2 x 10 at 250°c a) Which direction will rxn...
R-0.08206 (atm - L)(mol - K)= 8.314 J/(mol-K) pH = -log[H30) pOH = -log(OH) pX=-logX [HO'] = 10 Ph. K, EK.(RT) pH +...
R-0.08206 (atm - L)(mol - K)= 8.314 J/(mol-K) pH = -log[H30) pOH = -log(OH) pX=-logX [HO'] = 10 Ph. K, EK.(RT) pH + pOH = 14 = pK+pKb [OH (H:0= 10-14 = K, * Ks (in water at 25°C) pH =pK, + log([base)/(acid]) pOH =pKy + log (acid]/[base]) Molar Solubility = (*+ m for a salt that dissociates into ions with coefficients of n and m - b b -4ac where 0 = ax + bx+c VA= A/ X=- 1)...
Q29
What are the respective concentrations (M) of Cu^2+ and CI^- afforded by dissolving 0.741 mol CuCl_2 in water and diluting to 726mL? 0.00102 and 1.02 1.02 and 2.04 1.02 and 1.02 0.980 and 0.269 0.00102 and 0.00102
What are the respective concentrations ( M ) of Fe^3+ and 1 afforded by dissolving 0.200 moI Fel3 In 725 mL of water?
Calculate the pH of a solution that is prepared by dissolving 0.297 mol of pentafluorobenzoic acid (CF.COOH, K, -3.30x10-2) and 0.650 mol of hydrocyanic acid (HCN, K, = 6.17x10-10) in water and diluting to 5.90 L. Also, calculate the equilibrium concentrations of C F COOH, C F C00", HCN, and CN. Do not make an approximation unless the initial acid concentration is greater than 1000 × K. (Hint: The pH will be determined by the stronger acid of this pair.)...
please help me please i dont
have questions remaining anymore
A solution is prepared by dissolving 0.060 mol of iodoacetic acid (Kg = 6.68x10-4) and 0.040 mol of sodium iodoacetate in water to a total solution volume of 1.00 L. First, calculate a pH for the solution by assuming that the concentrations of ICH CO2H and ICH CO2 are equal to the formal concentrations of the substances dissolved. Submit Answer Tries 0/5 Next, calculate the pH for the solution based...
2. What is the pH of a solution which is 0.25 M KHCO, if the K, for HCOs is 2.4 x 10*2 Calculate the concentrations of НЗО", ОН, NHs, and cr in a solution prepared by dissolving 535 g of NH4CI in enough water to make 5.00 × 102 miL of solution at 25 °C., for NII is 1.8 x io-s. Hint: Is the given ionization constant for NHs the correct value to use in your calculations?) 3.
A solution is prepared by dissolving 0.23 mol of formic acid and 0.27 mol of sodium formate in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. The pH does not increase drastically because the NaOH reacts with the present in the buffer solution. The K, of formic acid is 1.8 x 10+ A formic acid B. sodium formate C water D. sodium E....
3.355 M K2SO4 solution can be prepared by A) dilution of 500.0 mL of 1.00 MK2SO4 to 1.00 L B) dissolving 46.7 g of K2SO4 in water and diluting to 500.0 ml, then diluting 25.0 ml of this solution to a total volume of 500.0 mL C) dissolving 46.7 g of K2SO4 in water and diluting to a total volume of 250.0 mL D) dilution of 1.00 mL of 0.355 M K2SO4 to 1.00 L E) diluting 46.7 mL of...
Bral -6.3 x 102 M & (Br)-1.2 x10 M. What are the equilibrium concentrations of Br, & Br at 1280C where K, 1.1 x 10'? Show ALL work (hint: test Q first) 9) Calculate (CoL,[Ch] & [COCk] when 5.00 mol COCI, decomposes&reaches equilibrium in 10.Ol flask. K 8.3 x 10* at 360°C 10) Reaction of 0.1050 mol PCl, w/0.0450 mol Cl, & 0.0450 mol PCl, in 0.5000 L flask. K, 4.2 x 10 at 250°c a) Which direction will rxn...
R-0.08206 (atm - L)(mol - K)= 8.314 J/(mol-K) pH = -log[H30) pOH = -log(OH) pX=-logX [HO'] = 10 Ph. K, EK.(RT) pH + pOH = 14 = pK+pKb [OH (H:0= 10-14 = K, * Ks (in water at 25°C) pH =pK, + log([base)/(acid]) pOH =pKy + log (acid]/[base]) Molar Solubility = (*+ m for a salt that dissociates into ions with coefficients of n and m - b b -4ac where 0 = ax + bx+c VA= A/ X=- 1)...
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