does 50mL of .1 M Ascorbic acid and 50 mL .1 M Sodium Alginate form a...

does 50mL of .1 M Ascorbic acid and 50 mL .1 M Sodium Alginate form a buffer? Ka is 6.3x10^-5. Will the pH change if 10 mL of .1 MNaOH is added, if so, what is the pH. please explain the answer

Expert Solution

queen_honey_blossom answered 2 years ago

You are titrating 25 mL of 0.25 M Ascorbic Acid solution ith 0.15 M NaOH. Ascorbic...

You are titrating 25 mL of 0.25 M Ascorbic Acid solution ith 0.15 M NaOH. Ascorbic Acid is an organic diprotic acid, H2A, that is found in many natural materials. Ka1 = 7.94 x 10^-5 and Ka2 = 1.62 x 10^-12. What is the a) initial pH, b) at the 1st equivalence point, c) the 2nd equivalence point, and d) after 27.5 mL of NaOH have been added?

You are titrating 50 ml. of nitrous acid with sodium hydroxide (0.15 M). Equivalence is reached...

You are titrating 50 ml. of nitrous acid with sodium hydroxide (0.15 M). Equivalence is reached at 22.0 ml of NaOH delivered. Calculate the pH of the solution in the flask: - before the beginning of the titration - after the delivery of 5 ml. of titrant - at half$equivalence - at equivalence -after delivery of 23 ml. of titrant. -------------Give detail Show ALL WORK, UNITS and use ICE/reaction table and ML (no millimoles). Please be clear in how you...

A vitamin C (ascorbic acid) tablet was dissolved in approximately 50 mL of distilled water and...

A vitamin C (ascorbic acid) tablet was dissolved in approximately 50 mL of distilled water and titrated with the standardized NaOH solution. From the results of this titration, the mg of ascorbic acid in the tablet was calculated. Molecular formula of ascorbic acid: C6H8O6 Volume of NaOH required to neutralize ascorbic acid in Vitamin C tablet (mL) 14.47 Concentration of NaOH in mol/L, 0.1964 Calculate the amount of ascorbic acid in the Vitamin C tablet in (mg).

Consider the titration of 40.0 mL of 0.523 M ascorbic acid (H2C6H6O6) with 0.885 M potassium...

Consider the titration of 40.0 mL of 0.523 M ascorbic acid (H2C6H6O6) with 0.885 M potassium hydroxide (KOH): pKa1 = 4.10 pKa2 = 11.80 What is the solution pH before the titration begins? _________________ What is the pH at the first half-equivalence point? What is the pH at the first equivalence point? _________________ _________________ What is the pH at the second half-equivalence point? _________________ What is the pH at the second equivalence point? _________________ What is the pH when 70.0...

What is the pH of 50 ml of a 0.10M weak acid (Ka =1.0x10-5) plus 50ml...

What is the pH of 50 ml of a 0.10M weak acid (Ka =1.0x10-5) plus 50ml water? What is the pH of 50 ml 0.010M weak base plus 100ml water ? Kb =1.0x10-5. What is the pH of a solution, which is 0.10M in a weak acid, HA and 0.2M in NaA? Ka =1.0x10-5

1. A 100.0-mL sample of 0.500 M sodium hydroxide is titrated with 0.100 M nitric acid....

1. A 100.0-mL sample of 0.500 M sodium hydroxide is titrated with 0.100 M nitric acid. Calculate the pH after 400.0 mL of acid has been added. 2. A 1.0-L buffer solution contains 0.100 mol HCN and 0.100 mol LiCN. The value of Ka for HCN is 4.9 x 10-10. Because the initial amounts of acid and conjugate base are equal, the pH of the buffer is equal to pKa = -log (4.9 x 10-10) = 9.31. Calculate the new...

1) A 100.0-mL sample of 0.500 M sodium hydroxide is titrated with 0.100 M nitric acid....

1) A 100.0-mL sample of 0.500 M sodium hydroxide is titrated with 0.100 M nitric acid. Calculate the pH after 600.0 mL of the acid has been added. 2) A 100.0-mL sample of 0.100 M HCHO2 is titrated with 0.200 M NaOH. Calculate the pH after adding 30.00 mL of the base.

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