(iii) 5.0, 25.0, 50.0 and 100.0 g aliquots of MgCl2 were dissolved in 4 separate 250 ml samples of distilled water. Calculate [H30*] and the pH for each of the resulting solutions and comment on the relationship between [MgCl2] and pH.
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![(iii) 5.0, 25.0, 50.0 and 100.0 g aliquots of MgCl2 were dissolved in 4 separate 250 ml
samples of distilled water. Calculate [H30*] and the pH for each of the resulting
solutions and comment on the relationship between [MgCl2] and pH.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1c62c0c4-eff4-4722-9e83-2ba901958293%2F4cdeeb3f-a6b5-4078-a5d5-33f7df6867ca%2Fh5349on_processed.jpeg&w=3840&q=75)
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- During the course of the titration of a 20.0 ml of solution containing 0.1 M of NaOH and 0.08 M of hydrazine (NH2-NH2) (Ka = 1.05 x 10) by a 0.2 M standard perchloric acid (HC104) titrant, calculate the pH of the titration mixture after (a) 5.0 ml; (b) 10.0 ml; and (c) 15.0 ml of HC1O4 titrant is added.a) What mass of Fe(NH4)2(SO4)2•2H2O(s) is required to prepare a 500 mL solution containing 100 ppm (m:v) in Fe? b) Using this stock solution, what aliquot must be used to prepare calibration solutions, 100 mL volume, of the following concentrations: 0.100 ppm, 0.500 ppm, 2.00 ppm, 4.00 ppm, and 7.00 ppm.An alkaline sample of sodium compounds weighing 1.196 g was dissolved in water, cooled to 15°C, treated with 2 drops of Pp indicator and titrated with 1.058 N H2SO4 requiring 6.8 ml to render the solution colorless. Upon adding 2 drops of MO and continuing the titration, 16.5 ml more of the acid were needed to complete the analysis. What is the quantitative composition of the sample? MW: NaOH = 40.0, Na2CO3 = 106.0, NaHCO3 = 84.01
- A biochemical reaction takes place in a 1.00 ml solution of 0.0250 Mphosphate buffer initially at pH = 7.20 (as shown for pKas of phosphatespecies).(a) Are the concentrations of any of the four possible phosphate speciesnegligible? If so, identify them and explain your answer.(b) During the reaction, 3.80 μmol of HCl are produced. Calculate the finalpH of the reaction solution. Assume that the HCl is completely neutralizedby the buffer.A sample of 0.10 M CH3COOH(aq) of volume 25.0 cm3 is titrated with 0.10 M NaOH(aq). The Ka for CH3COOH is 1.8 x 10-5. (a) What is the pH of 0.10 M CH3COOH(aq)? (b) What is the pH after the addition of 10.0 cm3 of 0.10 MNaOH(aq)? (c) What volume of 0.10 M NaOH(aq) is required to reach halfway to the stoichiometric point? (d) Calculate the pH at that halfway point. (e) What volume of 0.10 M NaOH(aq) is required to reach the stoichiometric point? (f) Calculate the pH at the stoichiometric point.2.413 g sample contains Na2CO3, NaHCO3 and inert material. This sample was solved in water and diluted to 250.0 ml. 80 ml solution was taken and titrated with 0.09644 N HCl with the indicator of phenolftalein. 6.13 ml HCl was consumed. From a second solution, again 80 ml was taken and titrated with the same HCl solution with the indicator of methylorange. 15.4 ml HCl was consumed. Calculate the percentage of NaHCO3 and Na2CO3in sample (Na2CO3=106.0 g/mol, NaHCO3=84.02 g/mol).
- 2.413 g sample contains Na2CO3, NaHCO3 and inert material. This sample was solved in water and diluted to 250.0 ml. 80 ml solution was taken and titrated with 0.09644 N HCl with the indicator of phenolftalein. 6.13 ml HCl was consumed. From a second solution, again 80 ml was taken and titrated with the same HCl solution with the indicator of methylorange. 15.4 ml HCl was consumed. Calculate the percentage of NaHCO3 and Na CO in sample (Na CO =106.0 g/mol, NaHCO =84.02 g/mol)(a) Sodium acetate, CH3COONA was hydrolysed in water, H2O. Show the reaction equations involved. What is the effect of the salt on the pH of this solution? (b) (i) Define buffer solution. (ii) 2.50 g of sodium acetate, CH3COONA was dissolved in 150.0 mL of water, H2O. A solution of 0.025 M ethanoic acid, CH3COOH was added into the above salt solution. Calculate the pH of the mixed solution. [pKa of CH3COOH = 4.75, Molar mass of CH3COONA = 82.0 g mol-1] (c) Explain how the above buffer solution maintain its pH when a small amount of sodium hydroxide, NaOH is added.(4) The amount of oxalic acid in a sample of 3+ rhubarb was determined by reacting with Fe as outlined in the following reaction. In a typical analysis, the oxalic acid in 10.62 g of rhubarb was extracted with a suitable solvent. The complete oxidation of the oxalic acid to 3+ CO, required 36.44 mL of 0.013 M Fe*.What is the weight percent of oxalic acid in the sample of rhubarb? 2FE3" (aq) + H2C,O,(aq) + 2H2O(1) → 2Fe?* (aq) + 2C02(g) + 2H;0 (aq)
- The phosphate in a 3.000-g sample of industrial detergent was precipitated by the addition of 1.000 g of AgNO3. The solution was filtered and filtrate, upon addition of 1.00 mL of 0.01 M fecl3, required 18.23 mL of 0.1377 M KSCN for titration to the end point. (a) the weight percent of phosphate in the detergent(iv) The Ksp for zinc oxide is 3.5 x 1017. What concentration of zinc sulfate (in mol/L) must be dissolved in water in contact with solid zinc oxide to obtain a solution pH of 5.9?.Write the balance equation of aqueous Pb(ClO3)2 with NaI. Include phases.