Using a pH 10 buffer solution of aqueous ammonia and aqueous ammonium chloride, for what reason...

Using a pH 10 buffer solution of aqueous ammonia and aqueous ammonium chloride, for what reason are we buffering the solution to be basic? What would happen to the structure of EDTA without a buffer? Explain how this would affect titration.

Solutions

Expert Solution

form of EDTA exists at pH=10 which is required for titration that's buffering is done.

Because at lower pH values form exists and this doesn't give result in titration.

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

Using a pH 10 buffer solution of aqueous ammonia and aqueous ammonium chloride, which chemical species...

Using a pH 10 buffer solution of aqueous ammonia and aqueous ammonium chloride, which chemical species is the weak base? Which is the conjugate acid? How do you know?

A buffer solution is made by dissolving .17g of ammonia and 1.07g ammonium chloride in enough...

A buffer solution is made by dissolving .17g of ammonia and 1.07g ammonium chloride in enough water to make 250mL of solution Detemine molarity of ammonium chloride Detemine ammonium concentration Determin solution molarity relative to ammonia Determine solution pH

To 160.0 mL of a buffer solution containing 0.250 M ammonia and 0.100 M ammonium chloride,...

To 160.0 mL of a buffer solution containing 0.250 M ammonia and 0.100 M ammonium chloride, 20.00 mL of 1.00M HClO4 are added. a) Calculate the pH of the initial buffer solution. b) Calculate the pH of the new solution after the addition of acid. c) What becomes the pH if another 20.00 mL of the same acid solution is added?

To 160.0 mL of a buffer solution containing 0.250 M ammonia and 0.100 M ammonium chloride,...

A buffer solution contains 0.424 M ammonium chloride and 0.235 M ammonia. If 0.0297 moles of...

A buffer solution contains 0.424 M ammonium chloride and 0.235 M ammonia. If 0.0297 moles of potassium hydroxide are added to 225 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume change does not change upon adding potassium hydroxide) pH = A buffer solution contains 0.382 M nitrous acid and 0.466 M potassium nitrite. If 0.0176 moles of hydrobromic acid are added to 150. mL of this buffer, what is the pH...

A) What is the pH of a 3.15×10-2 M aqueous solution of ammonium iodide, NH4I ?...

A) What is the pH of a 3.15×10-2 M aqueous solution of ammonium iodide, NH4I ? The solution is ________. (acidic, basic, neutral) B)The substance benzoic acid (C6H5COOH) is a weak acid (Ka = 6.3×10-5). What is the pH of a 0.101 M aqueous solution of sodium benzoate, NaC6H5COO? The solution is ________.(acidic, basic, neutral)

What is the pH of a 0.124 M aqueous solution of ammonium iodide, NH4I ? pH...

What is the pH of a 0.124 M aqueous solution of ammonium iodide, NH4I ? pH = This solution is _________ (acidic, basic, or neutral)

Activity 4: Equilibrium of solid ammonium chloride with ammonium chloride in aqueous solution. NH4Cl(s) +H2O(l) ...

Activity 4: Equilibrium of solid ammonium chloride with ammonium chloride in aqueous solution. NH4Cl(s) +H2O(l)  NH4+(aq) + Cl-(aq) (ammonium chloride) (ammonium ion) Procedure * Pour about 75 mL of tap water into a 150-mL beaker and heat to boiling on a hot plate. * While waiting for the water to boil, place approx. 1 mL of a saturated NH4Cl solution into a small, clean, dry test tube. *To this test tube, add concentrated HCl solution one drop at a...

a) A buffer contains significant amounts of both ammonia (NH3) and ammonium chloride (NH4Cl). Write the...

a) A buffer contains significant amounts of both ammonia (NH3) and ammonium chloride (NH4Cl). Write the net ionic equation showing how this buffer neutralizes added HI. Express your answer as a chemical equation. b)A buffer contains significant amounts of both ammonia (NH3) and ammonium chloride (NH4Cl). Write the net ionic equation showing how this buffer neutralizes added NaOH. Express your answer as a chemical equation.

The pH of an aqueous solution of 7.96×10-2 M ammonium nitrate, NH4NO3 (aq), is . This...

The pH of an aqueous solution of 7.96×10-2 M ammonium nitrate, NH4NO3 (aq), is . This solution is

Subjects