Calculate the weight of citric acid – H2O (MW = 210 g/mol) and NaOH (MW 40g/mol)...
Calculate the weight of citric acid – H2O (MW = 210 g/mol) and NaOH (MW 40g/mol) needed to prepare 1.0 L of citrate buffer which is 0.2 M in Na+ and pH 5.2 (pK1= 3.13, pK2= 4.76, pK3= 6.4.
Answers:
24.2 g citric acid – H2O and 8.0 g NaOH
Homework Answers
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Calculate the weight of citric acid – H2O (MW = 210 g/mol) and
NaOH (MW 40g/mol)...
Citric Acid has 3 pKas: 3.13, 4.76, and 6.39. How many grams of sodium citrate monobasic...
Citric Acid has 3 pKas: 3.13, 4.76, and 6.39. How many grams of sodium citrate monobasic (HOC(COONa)(CH2COOH)2) and citric acid (HOC(COOH)(CH2COOH)2) are needed to make 300 mL of a 10 mM citrate buffer of exactly pH 2.8? The molecular weight of sodium citrate monobasic (NaH7C6O7) is 214.11 g/mol and that of citric acid (H8C6O7) is 192.12 g/mol.
Calculate the molar ratio of citric acid and sodium citrate required to prepare 40mM buffer pH...
Calculate the molar ratio of citric acid and sodium citrate required to prepare 40mM buffer pH 4.8 citric acid pka= 3.13, 4.76, 6.39
Question 3 10 pts 1.0 L of buffer solution is made from 0.17 mol citric acid...
Question 3 10 pts 1.0 L of buffer solution is made from 0.17 mol citric acid and 0.11 mol sodium citrate. After adding 0.25 mol HCl to the buffer, what is the pH? Ignore the volume change. K, citric acid - 8.4e-4
7. A 0.653 g of a monoprotic solid acid (mw= 157 g/mol) is dissolved in water...
7. A 0.653 g of a monoprotic solid acid (mw= 157 g/mol) is dissolved in water to produce a 50.0 mL solution. The pH of this solution is measure to be pH = 2.13. Determine the ionization constant (Ka) of the acid. 8. A buffer is 0.50 M CH3COOH(aq) and 0.50 M Na(C6H-C00) (aq). For CH2COOH pKa = 4.20 a) Calculate the pH of the buffer solution. b) Calculate the pH after the addition of 40 mL of a 0.150...
You are asked to prepare 500. mL of a 0.100 M acetate buffer at pH 5.00 using only pure acetic acid (MW=60.05 g/mol,...
You are asked to prepare 500. mL of a 0.100 M acetate buffer at pH 5.00 using only pure acetic acid (MW=60.05 g/mol, pKa=4.76), 3.00 M NaOH, and water. Answer the following questions regarding the preparation of the buffer. 1. How many grams of acetic acid will you need to prepare the 500 mL buffer? Note that the given concentration of acetate refers to the concentration of all acetate species in solution. 2. What volume of 3.00 M NaOH must...
A 1.18 M solution of citric acid (H3C6H507, MW=192.122 g/mol) in water has a density of...
A 1.18 M solution of citric acid (H3C6H507, MW=192.122 g/mol) in water has a density of 1.8 g/mL. What is the mass percent of this solution? Select one: a. 75.42% O b. None of the choices is correct c. 3.93% Od. 12.59 % O e. 68.21 %
What weight of dry sodium acetate (FW = 82 g/mol) and volume of acetic acid (MW...
What weight of dry sodium acetate (FW = 82 g/mol) and volume of acetic acid (MW = 60 g/mol; density = 1.049 ml/g are required for 1 liter of 0.1 M sodium acetate, pH 4.50. (pKa= 4.73)? Answer: 3.6 mL acetic acid, 3.0 g sodium acetate Please provide steps to get the above answer.
1.Calculate the mass of malonic acid (C3H4O4, MW 104.07 g/mol) required to prepare 50.00mL of a...
1.Calculate the mass of malonic acid (C3H4O4, MW 104.07 g/mol) required to prepare 50.00mL of a 0.15 M malonic acid solution. 2. Calculate the mass of manganese sulfate monohydrate (MnSO4*H2O, MW 169.01 g/mol) required to prepare 50.00mL of a 0.020 M manganese sulfate solution 3. Calculate the mass of potassium iodate (KIO3,MW 213.99 g/mol) required to prepare 50.00mL of a 0.20 M potassium iodate solution. 4. Calculate the volume of 1.0 M sulfuric acid (H2SO4) required to prepare 100.00mL of...
1. Please calculate the pH of a solution containing 2.0M citric acid and 1.0M sodium citrate....
1. Please calculate the pH of a solution containing 2.0M citric acid and 1.0M sodium citrate. 2. Please calculate the pH of a solution containing 1.0M tartaric acid and 1.OM potassium tartarate. 3. Please calculate the pH of a solution containing 0.25M CH NH, and 0.37M C.HNH,CI. 4. Please design a buffer system to maintain a pH of 7.20. 5. Please design a buffer system to maintain a pH of 3.70. 6. For each of the following solutions please calculate...
Calculate the mass of solid formic acid (MM = 46.0 g/mol - Ka = 1.8 x...
Calculate the mass of solid formic acid (MM = 46.0 g/mol - Ka = 1.8 x 10-4 ) and sodium formate (MM = 68 g/mol) needed to make 100 mL a 0.2 M formic acid buffer that is 1:3 (conjugate base/weak acid). Also predict the pH of this buffer.
Question 3 10 pts 1.0 L of buffer solution is made from 0.17 mol citric acid and 0.11 mol sodium citrate. After adding 0.25 mol HCl to the buffer, what is the pH? Ignore the volume change. K, citric acid - 8.4e-4
7. A 0.653 g of a monoprotic solid acid (mw= 157 g/mol) is dissolved in water to produce a 50.0 mL solution. The pH of this solution is measure to be pH = 2.13. Determine the ionization constant (Ka) of the acid. 8. A buffer is 0.50 M CH3COOH(aq) and 0.50 M Na(C6H-C00) (aq). For CH2COOH pKa = 4.20 a) Calculate the pH of the buffer solution. b) Calculate the pH after the addition of 40 mL of a 0.150...
A 1.18 M solution of citric acid (H3C6H507, MW=192.122 g/mol) in water has a density of 1.8 g/mL. What is the mass percent of this solution? Select one: a. 75.42% O b. None of the choices is correct c. 3.93% Od. 12.59 % O e. 68.21 %
1. Please calculate the pH of a solution containing 2.0M citric acid and 1.0M sodium citrate. 2. Please calculate the pH of a solution containing 1.0M tartaric acid and 1.OM potassium tartarate. 3. Please calculate the pH of a solution containing 0.25M CH NH, and 0.37M C.HNH,CI. 4. Please design a buffer system to maintain a pH of 7.20. 5. Please design a buffer system to maintain a pH of 3.70. 6. For each of the following solutions please calculate...
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