0.1 g of the mixture of na2so4 and k2so4 is taken and 100 ml of solution is prepared. 10 ml of this prepared solution is placed in a beaker and some distilled water is added. A mass of 15.5 mg is obtained by precipitation with Bacl2 at PH=5, then filtering and bringing to a constant weight at 800 °C. Calculate the percentages of Na2so4 and K2so4 in the mixture accordingly.

0.1 g of the mixture of na2so4 and k2so4 is taken and 100 ml of solution is prepared. 10 ml of this prepared solution is placed in a beaker and some distilled water is added. A mass of 15.5 mg is obtained by precipitation with Bacl2 at PH=5, then filtering and bringing to a constant weight at 800 °C. Calculate the percentages of Na2so4 and K2so4 in the mixture accordingly.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 107AP

See similar textbooks

Similar questions

b. A student has a sea water sample which contains Ca2+ ions . Describe briefly how he willdetermine the concentration of Ca2+ ion in the sample using a simple titration. Explain the colourchanges at the endpoint. Which medium is suitable for performing the titration, acidic or basic medium and why?
A 250 cm3 volumetric flask contains exactly 200,0 cm3 of a 0,025 mol.dm3sulphuric acid solution. Thereafter ten (10) sodium hydroxide pellets, eachof mass 0,1 g are dropped into the flask. After the pellets have dissolvedcompletely, the flask is topped to the 250 cm3 mark with water and thecontents are thoroughly homogenised. Determine the pH of the resultingsolution.
a) At temperature 25°C, 0.02 M hydrazine, N2H4 solution is 0.69% ionised. Calculate the i. Concentration of OH- ion ii. ionisation constant, Kb b) Calculate the mass of sodium benzoate, C6H5COONa that should be added to 500 mL of 0.2M aqueous benzoic acid, C6H5COOH solution to produce a buffer with pH 3.50?[ Ka for C6H5COOH = 6.3 x10-5] c) When a 1 x 10-3 moldm-3 solution of CaCl2 is mixed with an equal volume of a 1 x 10-3 moldm-3 solution of Na2SO4, will precipitate form? (Ksp CaSO4= 2 x 10-5) Do you mean that pH? That was all the given information the question gave.. I don't understand how to use the ionised part the most
) A truck driver carrying a load of lead nitrate (Pb(NO3)2) lost control of his semi- truck after hitting a patch of ice and crashed the truck into Blue Lake, which was right next to the highway. Despite the best efforts of the emergency workers, several of the crates containing lead nitrate were damaged, and the highly soluble compound dissolved immediately. Assuming the lake is initially at circumneutral pH (7), and that the spill resulted the in a total lead concentration of 10-3 M within the lake. Based on the following information, will PbO(s) precipitate out of Blue Lake. Assume all lead nitrate dissociates into Pb+2 and NO3-, no other sources of lead exist in the lake and that no other reactions besides the equations shown below occur. PbO(s) + 2H+ ⇌ PbO(s) + H+ ⇌ PbO(s) + H2O ⇌ PbO(s) + 2H2O ⇌ Pb2+ + H2O PbOH+ + H2O Pb(OH)2o Pb(OH)3- + H+ logKs0/ksp =14 logK1=3.4 logK2=-0.5 logK3=-12
For the adjustment of 0.1 M HCl standard solution, 0.1345 g Na2CO3 in primary standard purity was weighed, dissolved in 50 mL of distilled water and titrated with HCl solution. As a result of the titration, 14 mL of acid solution was consumed. Accordingly, what is the true concentration of the HCl solution?
In developing a method for the determination of formic acid by neutralization volumetry, an analyst calculated the pH as a function of the addition of NaOH for the titration of 30.00 mL of 0.1280 mol/L formic acid with standardized NaOH with concentration of 0.1570 mol/L. With respect to this titration curve, determine the pH of the solution after adding the following volumes of NaOH: 0.00 mL; 10.00 ml; 25 mL of titrant and at the equivalence point. Data: Ka=1.70x10-4. Present the results with two decimal places and show your calculations.
Consider exactly one litre of a propanoic acid buffer solution, containing 0.600 M C3H5OOH and 0.252 M C3H5OO- . 1.1 Determine the pH of the buffer solution. - You may use “HA” to denote the formula of the acid. - You may make certain assumptions to simplify your calculations - Ka for hydrofluoric acid is 1.3 × 10−5 . 3.2 Determine by means of a full calculation the change in pH of the buffer solution that will result when 100. mL of a 1.00 × 10−2 M HCℓ solution is added to it. You must indicate all the relevant reaction equations in your working.
Consider the reaction of 75.0 mL of 0.350 M C₅H₅N (Kb = 1.7 x 10⁻⁹) with 100.0 mL of 0.425 M HCl. With 0.0162 moles of H⁺ in excess in a volume of 175.0 mL, what would be the pH of this solution after the reaction?
An approximately 0.1-molar solution of NaOH is to be standardized by titration. Assume that the following materials are available. Clean, dry 50 mL buret •Analytical balance 250 mL Erlenmeyer flask •Wash bottle filled with distilled water Phenolphthalein indicator solution Potassium hydrogen phthalate, KHP, a solid monoprotic acid (to be used as the primary standard) Briefly describe the steps you would take, using the materials listed above, to standardize the NaOH solution. Describe (the set up) the calculations necessary to determine the concentration of the NaOH solution.
One drop, 0.200 cm3, of 1.00 mol dm-3 of aqueous sodium hydroxide, NaOH, solution is added to 25.0 cm3 of a phosphate buffer that is 0.040 mol dm-3 in KH2PO4(aq) and 0.020 mol dm-3 in K2HPO4(aq). Calculate the resulting pH of the solution given that the second acid dissociation constant, pKa2, for phosphoric acid is 7.21.
A chemist who works in the process laboratory of the Athabasca Alkali Company makes frequent analyses of ammonia recovered from the Solvay process for making sodium carbonate. What is the pH at the equivalencepoint if she titrates the aqueous ammonia solution (approximately 0.10 M) with a strong acid of comparable concentration? Select an indicator that would be suitable for the titration.
Suppose someone did not put enough 3M HCl in a beaker and conducted a filtration of the cloudy suspension when the pH was 4 rather than 2. A very low yield of product was obtained after drying and filtration of the solid. Suggest possible reasons for this lower yield.