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Titration of 0.1756g of the primary standard Na,C,0, required 32.04 mL of a potassium permanganate solution....
equilibnum M27 Calculate the hydrogen ion concentration of a solution that is 0.05 M in potassium...
equilibnum M27 Calculate the hydrogen ion concentration of a solution that is 0.05 M in potassium hydrogen phthalate, KHP, and 0.15 M in potassium phthalate, KzP. Phtalic acid: Ka, = 1.12x10-3; Ka, = 3.90x10-6
diculate the hydrogen ion concentration of a solution that is 0.05 M in potassium hydrogen phthalate,...
diculate the hydrogen ion concentration of a solution that is 0.05 M in potassium hydrogen phthalate, KHP, and 0.15 M in potassium phthalate, K2P. Phtalic acid: Ka, = 1.12x10-3; Ka, = 3.90x10-6
6. Titration of a 50.00 mL solution of an unknown diprotic acid required 35.95 mL of...
6. Titration of a 50.00 mL solution of an unknown diprotic acid required 35.95 mL of 0.1367 M sodium hydroxide to reach the second equivalence point. What was the initial concentration of the unknown acid . A 0.8752 g sample of unknown containing potassium hydrogen phthalate (KHP) required 28.23 mL of a 0.1037 M NaOH for neutralizatjon. What is the mass percentage of KHP in the sample?
3. A solution is prepared by treating 50 mL of 0.50 M HF (Ka = 6.6x10...
3. A solution is prepared by treating 50 mL of 0.50 M HF (Ka = 6.6x10 ) with 10 mL of 1.15 M NaOH. Calculate the pH of the solution. 4. If enough NaOH is added to the solution in problem 3 to neutralize the HF, what will the pH be? 5. 42.16 mL of a solution of NaOH are required to neutralize 0.7878 g of potassium hydrogen phthalate (Mwt = 204.23 g/mol). Calculate the molar concentration of NaOH in...
n a pink aqueous solution of potassium permanganate, faintly addified with dilute sulfuric acid was treated the reaction took place with the evolution of gas bubbles, and the pink solution turned...
n a pink aqueous solution of potassium permanganate, faintly addified with dilute sulfuric acid was treated the reaction took place with the evolution of gas bubbles, and the pink solution turned colorless. Further chemical analysis revealed that the evolved gas was oxygen, and the resulting solution contains potassium sulfate and manganese () sulfate; water was also formed during the same reaction. Please with 10% aq. hydrogen peroxide, answer the followings: 1) Write down the balanced chemical equation for this reaction....
Weak Acid-Strong Base Titration Date Nanse PRE-LAB OUESTIONS 1 Calculate the molarity of a NaOH solution...
Weak Acid-Strong Base Titration Date Nanse PRE-LAB OUESTIONS 1 Calculate the molarity of a NaOH solution that was used to titrate 1.2 g of potassium acid phthalate if 37.50 ml of the base were reauired to get to the end point of the titration. 2 It takes 12.45 ml. of a 0.500 M NaOH solution larity of the acid to titrate 30.0 mL of acetic acid. What is the mo- 3. Using the titration curve below, calculate the K, of...
1. Calculate the volume (in mL) of the amount of 0.200 M NaOH required to neutralize...
1. Calculate the volume (in mL) of the amount of 0.200 M NaOH required to neutralize a monoprotic weak acid solution made by 2.00 g of potassium hydrogen phthalate (KHP) dissolved in water. Hint: the complete neutralization occurs at the equivalence point, where the number of moles of the analyte (in this case, the weak acid) equal to the titrant (in this case, the strong base). 2. Identify the equivalence point, the half-equivalence point on the titration curve below and...
C.)2.6 d.) 423 3. Calculate the concentration of a murexide solution with an absorbance of 528...
C.)2.6 d.) 423 3. Calculate the concentration of a murexide solution with an absorbance of 528 at 540 nm given that a 2.75 x 10A-4 M solution has an absorbance of .487 at 540 nm a. 2.98 x 10A-4 M B.) 3.35 x 10A3 M .)9.64 x 10 A-7 d.12.54 x 10 4 4. Calculate the equilibrium constant for the reaction Fe3+ (ago+SCN (aq) FescN2+ (aq) given that the mixture of 5 ml of.00359 M SCN- and 5 ML of...
Suppose 1.00 g of NaOH is used to prepare 250 mL of an NaOH solution. Compare...
Suppose 1.00 g of NaOH is used to prepare 250 mL of an NaOH solution. Compare the expected molarity of this solution to the actual average molarity you measured in the standardization. What do you notice? Do you think the results would have been more accurate if a different type of acid or base were used in the standardization? Why, or why not? There are many different primary standards that could be used in a standardization titration. What are the...
A chemistry teacher needs to make 2.30 L of a potassium chloride solution for an experimen...
A chemistry teacher needs to make 2.30 L of a potassium chloride solution for an experimen The concentration of the required solution is 3.10 M. How many grams of KCI will she need to use? 0 7.13 g KCI 0 231 g KCI O 532 g KCI 0.0956 g KCI What is the equation for the ion product constant of water at 25 °C? Kw [H,0+][OH-] [H,O] = 1.00 x 10-14 Kw [H,0+1 [OH-] = 1.00 x 10-14 Kw =...
equilibnum M27 Calculate the hydrogen ion concentration of a solution that is 0.05 M in potassium hydrogen phthalate, KHP, and 0.15 M in potassium phthalate, KzP. Phtalic acid: Ka, = 1.12x10-3; Ka, = 3.90x10-6
diculate the hydrogen ion concentration of a solution that is 0.05 M in potassium hydrogen phthalate, KHP, and 0.15 M in potassium phthalate, K2P. Phtalic acid: Ka, = 1.12x10-3; Ka, = 3.90x10-6
6. Titration of a 50.00 mL solution of an unknown diprotic acid required 35.95 mL of 0.1367 M sodium hydroxide to reach the second equivalence point. What was the initial concentration of the unknown acid . A 0.8752 g sample of unknown containing potassium hydrogen phthalate (KHP) required 28.23 mL of a 0.1037 M NaOH for neutralizatjon. What is the mass percentage of KHP in the sample?
3. A solution is prepared by treating 50 mL of 0.50 M HF (Ka = 6.6x10 ) with 10 mL of 1.15 M NaOH. Calculate the pH of the solution. 4. If enough NaOH is added to the solution in problem 3 to neutralize the HF, what will the pH be? 5. 42.16 mL of a solution of NaOH are required to neutralize 0.7878 g of potassium hydrogen phthalate (Mwt = 204.23 g/mol). Calculate the molar concentration of NaOH in...
n a pink aqueous solution of potassium permanganate, faintly addified with dilute sulfuric acid was treated the reaction took place with the evolution of gas bubbles, and the pink solution turned colorless. Further chemical analysis revealed that the evolved gas was oxygen, and the resulting solution contains potassium sulfate and manganese () sulfate; water was also formed during the same reaction. Please with 10% aq. hydrogen peroxide, answer the followings: 1) Write down the balanced chemical equation for this reaction....
Weak Acid-Strong Base Titration Date Nanse PRE-LAB OUESTIONS 1 Calculate the molarity of a NaOH solution that was used to titrate 1.2 g of potassium acid phthalate if 37.50 ml of the base were reauired to get to the end point of the titration. 2 It takes 12.45 ml. of a 0.500 M NaOH solution larity of the acid to titrate 30.0 mL of acetic acid. What is the mo- 3. Using the titration curve below, calculate the K, of...
1. Calculate the volume (in mL) of the amount of 0.200 M NaOH required to neutralize a monoprotic weak acid solution made by 2.00 g of potassium hydrogen phthalate (KHP) dissolved in water. Hint: the complete neutralization occurs at the equivalence point, where the number of moles of the analyte (in this case, the weak acid) equal to the titrant (in this case, the strong base). 2. Identify the equivalence point, the half-equivalence point on the titration curve below and...
C.)2.6 d.) 423 3. Calculate the concentration of a murexide solution with an absorbance of 528 at 540 nm given that a 2.75 x 10A-4 M solution has an absorbance of .487 at 540 nm a. 2.98 x 10A-4 M B.) 3.35 x 10A3 M .)9.64 x 10 A-7 d.12.54 x 10 4 4. Calculate the equilibrium constant for the reaction Fe3+ (ago+SCN (aq) FescN2+ (aq) given that the mixture of 5 ml of.00359 M SCN- and 5 ML of...
A chemistry teacher needs to make 2.30 L of a potassium chloride solution for an experimen The concentration of the required solution is 3.10 M. How many grams of KCI will she need to use? 0 7.13 g KCI 0 231 g KCI O 532 g KCI 0.0956 g KCI What is the equation for the ion product constant of water at 25 °C? Kw [H,0+][OH-] [H,O] = 1.00 x 10-14 Kw [H,0+1 [OH-] = 1.00 x 10-14 Kw =...
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