A 30.00-mL solution of HBr was treated with 5 mL of freshly boiled and cooled 8...

A 30.00-mL solution of HBr was treated with 5 mL of freshly boiled and cooled 8 M HNO3, and then with 50.00 mL of 0.3650 M AgNO3 with virgorous stirring. Then 1 mL of saturated ferric alum was added and the solution was titrated with .2870 M KSCN. When 3.60 mL had been added, the solution turned red. What was the concentration of HBr in the origninal solution? How many millimgrams of Br- were in the original solution?

Expert Solution

Ans is

queen_honey_blossom answered 1 year ago

A 30.00 mL sample of 0.0100M MgEDTA2- solution was added to a 30.00 mL sample containing...

A 30.00 mL sample of 0.0100M MgEDTA2- solution was added to a 30.00 mL sample containing Fe3+. The solution was then buffered to pH 10 and titrated with 12.83 mL of 0.0152 M EDTA to an Eriochrome Black-T endpoint. What was the [Fe3+] in the original sample? Please show work.

A 30.00 mL sample of 0.200 M HBr was titrated with 0.160 M KOH. a. What...

A 30.00 mL sample of 0.200 M HBr was titrated with 0.160 M KOH. a. What is the initial pH of the sample? b. What is the equivalence volume? c. What is the pH after 19.16 mL of KOH is added?

what is the pH of a solution that mixes 30.00 mL of 0.010 M Ch3oh with...

what is the pH of a solution that mixes 30.00 mL of 0.010 M Ch3oh with 30.00 mL 0.00750 M Nach3co2?

A 0.400 g sample of toothpaste was boiled with a 25 ml solution TISAB buffer to...

A 0.400 g sample of toothpaste was boiled with a 25 ml solution TISAB buffer to extract the fluoride. After cooling, the solution was diluted to exactly 100.0ml with more TISAB solution. The potential of fluoride ion-selective electrode/reference electrode in an aliquot of the sample was measured to be 186.6 mV. This value corresponding to a log[F-] of -3.5016 on a working curve of mV versus log [F-]. Calculate the weight percent F- and NaF in the toothpaste sample.

Determine the pH of the solution when 30.00 mL of 0.2947 M NH3 is titrated with...

Determine the pH of the solution when 30.00 mL of 0.2947 M NH3 is titrated with 10.00 mL of 0.4798 M HCl.

25.0 mL of 0.200 M solution of HBr are mixed with 25.0 mL of 0.200 M...

25.0 mL of 0.200 M solution of HBr are mixed with 25.0 mL of 0.200 M solution of NaOH in a constant pressure calorimeter. The temperature increases from 23.00 °C to 24.37 °C. Assume that the specific heat of the solution is the same as that of pure water (4.18 J/(g•°C)) and that the density is the same as pure water (1.00 g/mL). Calculate ΔH per mole of reaction for the below chemical reaction. HBr (aq) + NaOH (aq) →...

Calculate the pH of a 2.30×10-8 M solution of HBr.

calculate the pH of a 4.20x10^-8 M solution of HBr with water

A 30.00 mL solution of 0.235 M CH2NH2 was titrated with 0.150 M H2SO4. a) Calculate...

A 30.00 mL solution of 0.235 M CH2NH2 was titrated with 0.150 M H2SO4. a) Calculate the pH of the 30.00 mL solution of 0.235 M CH2NH2 b) Calculate the volume of 0.150 M H2SO4 required to neutralize the 30 mL solution of 0.235 M CH2NH2. c) Calculate the volume of 0.150 M H2SO4 required to neutralize half the mole of CH2NH2 present 30 Ml solution of 0.235 M CH2NH2 d) Calculte the pH of the solution in (c). e)...

A 1.000-mL aliquot of a solution containing Cu2 and Ni2 is treated with 25.00 mL of...

A 1.000-mL aliquot of a solution containing Cu2 and Ni2 is treated with 25.00 mL of a 0.03742 M EDTA solution. The solution is then back titrated with 0.02190 M Zn2 solution at a pH of 5. A volume of 20.48 mL of the Zn2 solution was needed to reach the xylenol orange end point. A 2.000-mL aliquot of the Cu2 and Ni2 solution is fed through an ion-exchange column that retains Ni2 . The Cu2 that passed through the...

Question