A 2.00 g sample of a powdered fruit drink containing citric acid, required 20.3 Ml of...

A 2.00 g sample of a powdered fruit drink containing citric acid, required 20.3 Ml of 0.113 M NaOH for complete neutralization. calculate the percent citric acid in the sample, Please show your work so i can understand.

Solutions

Expert Solution

C3H5O(COOH)3 (aq) + 3 NaOH(aq) --------------------> Na3C3H5O(COO)3(aq) + 3 H2O (l)

moles of NaOH = 20.3 x 0.113 / 1000 = 2.2939 x 10^-3

here

1 mol citric acid react -------------- 3 moles of NaOH

so moles of citric acid = moles of NaOH / 3

= 2.2939 x 10^-3 / 3

= 7.65 x 10^-4

molar mass of citric acid = 192.12 g/mol

mass 0f citric acid = moles x molar mass

= 7.65 x 10^-4 x 192.12

= 0.147 g

% citric acid = (0.147 / 2.00 ) x 100

= 7.34%

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

A biochemist dissolved 5.00 g citric acid in 250 mL of water. The pKa of citric...

A biochemist dissolved 5.00 g citric acid in 250 mL of water. The pKa of citric acid is 3.13 and the molecular weight is 192 g/mol. Determine the pH of the solution and the ratio of conjugate base to weak acid at equilibrium.

A fajans titration of a 0.9628 g sample containing chloride required 31.32 ml of 0.1001 M...

A fajans titration of a 0.9628 g sample containing chloride required 31.32 ml of 0.1001 M AgNO3. Express the result of this analysis in terms of the percent AlCl3 (FW= 133.34) in the sample.

7.36 g citric acid is dissolved in 1 L of its solution. 12.0 mL of this...

7.36 g citric acid is dissolved in 1 L of its solution. 12.0 mL of this solution is required to neutralize 15.0 mL of Ba(OH)2 solution. What is the molarity of the Ba(OH)2 solution? Also, find the grams of citric acid required to neutralize the base here 3Ba(OH)2(aq) + 2H3C6H5O7(aq) → Ba3(C6H5O7)2(aq) + 6H2O(l)

Calculate the pH of buffers based on the recipe: 13.16 g citric acid monohydrate 171 mL...

Calculate the pH of buffers based on the recipe: 13.16 g citric acid monohydrate 171 mL 1M NaOH 829 mL H2O --------------------------- Compound MW pKa if ionic strength =0 Citric acid monohydrate 210.14 g/mol 3.128, 4.761, 6.396

A 100.0 mL solution containing 0.830 g of maleic acid (MW = 116.072 g/mol) is titrated...

A 100.0 mL solution containing 0.830 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.298 M KOH. Calculate the pH of the solution after the addition of 48.0 mL of the KOH solution. Maleic acid has pKa values of 1.92 and 6.27. pH = At this pH, calculate the concentration of each form of maleic acid in the solution at equilibrium. The three forms of maleic acid are abbreviated H2M, HM–, and M2–, which represent the fully...

A 100.0 mL solution containing 0.8366 g of maleic acid (MW = 116.072 g/mol) is titrated...

A 100.0 mL solution containing 0.8366 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.3203 M KOH. Calculate the pH of the solution after the addition of 45.00 mL of the KOH solution. Maleic acid has pKa values of 1.92 and 6.27. At this pH, calculate the concentration of each form of maleic acid in the solution at equilibrium. The three forms of maleic acid are abbreviated H2M, HM–, and M2–, which represent the fully protonated, intermediate,...

A 100.0 mL solution containing 0.7590 g of maleic acid (MW = 116.072 g/mol) is titrated...

A 100.0 mL solution containing 0.7590 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.2906 M KOH. Calculate the pH of the solution after the addition of 45.00 mL of the KOH solution. Maleic acid has pKa values of 1.92 and 6.27. pH=? At this pH, calculate the concentration of each form of maleic acid in the solution at equilibrium. The three forms of maleic acid are abbreviated H2M, HM-, and M^2-, which represent the fully protonated,...

A 100.0 mL solution containing 0.753 g of maleic acid (MW = 116.072 g/mol) is titrated...

A 100.0 mL solution containing 0.753 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.259 M KOH. Calculate the pH of the solution after the addition of 50.0 mL of the KOH solution. Maleic acid has pKa values of 1.92 and 6.27. At this pH, calculate the concentration of each form of maleic acid in the solution at equilibrium. The three forms of maleic acid are abbreviated H2M, HM–, and M2–, which represent the fully protonated, intermediate,...

A 100.0 mL solution containing 0.756 g of maleic acid (MW = 116.072 g/mol) is titrated...

A 100.0 mL solution containing 0.756 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.217 M KOH. Calculate the pH of the solution after the addition of 60.0 mL of the KOH solution. Maleic acid has pKa values of 1.92 and 6.27. At this pH (pH = 9.48), calculate the concentration of each form of maleic acid in the solution at equilibrium. The three forms of maleic acid are abbreviated H2M, HM–, and M2–, which represent the...

A 100.0 mL solution containing 0.976 g of maleic acid (MW = 116.072 g/mol) is titrated...

A 100.0 mL solution containing 0.976 g of maleic acid (MW = 116.072 g/mol) is titrated with 0.296 M KOH. Calculate the pH of the solution after the addition of 56.00 mL of the KOH solution. Maleic acid has pKa values of 1.92 and 6.27 . pH = At this pH, calculate the concentration of each form of maleic acid in the solution at equilibrium. The three forms of maleic acid are abbreviated H2M, HM–, and M2–, which represent the...

Subjects