Using activity coefficients, calculate the pH of a solution containing a 2.00:1.00 mole ratio of HC² -:C³ – (H,C = citric acid). The ionic strength is 0,010 M. The pK, values for citric acid are 3.13, 4.76, and 6,40, pH = 5.846 What will be the pH if the ionic strength is raised to 0.10 M and the mole ratio HC²-:C³- is kept constant?
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- What is the pH of a 2.3 x 10-8 M solution of NaOH? You must consider the autodissociationof water at concentrations this low. Write the mass balance for sodium, charge balance, and the oneequilibrium expression. This will give three equations and three unknowns (Na+, H+, and OH-). Youcan assume all activity coefficients are 1 at an ionic strength this low. Bonus hint: The roots of thepolynomial are -1.1216 x10-7 and 8.9159 x10-82. If BaCl2 completely dissolves in water, what is the ionic strength of a 0.0300 F solution of BaCl2? 3. What is the pH of a solution that is 0.010 F HBr? 4. What is the pH of a solution that is 0.150 F in HBr? (You will need to use the Debye-Huckel equation to answer this.)10. 50 cm3 of 0.05 M weak acid solution is titrated with 0.1 M NaOH solution. The measured pH valuesare 7.345 and 7.497 at the consumptions of 6.0 and 6.1 cm3, respectively. What value of the buffer capacity can be calculated in the solution at pH = 7.421?11. Based on the data given in question 10, what is the total concentration of the anion of the weak acid atthe given point?
- 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 mostThe Ka values for nitrous acid (HNO2) and hypochlorous (HClO) acid are 4.5 x10-4and 3.0 x10-8, respectively. Which one would be more suitable for use in asolution buffered at pH = 7.0? What other substances would be needed to makethe buffer?Using a relevant ICE Table, calculate the expected pH of the solution when 4.81 mL of 0.200 M NaOH solution is added to the 50.0 mL of 0.100 M acetic acid HC2H3O2 solution. Compare the calculated value to the corresponding experimental value.
- 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?Calculate the alkaline strength of pearl ash (impure potassium carbonate) in terms of percent K2O from the following data: Sample = 0.3500 g; HCl used = 48.03 mL; NaOH used for back titration = 2.02 mL; 1.000 mL HCl = 0.005300 g Na2CO3; 1.000 mL NaOH = 0.02192 g KHC2O4.H2O. (Note: Use the least significant digits in your answer.)You have performed an iodimetric titration using a commercial vitamin C tablet. Based on the following information below, calculate the %(w/w) of vitamin C(MM=176.16 g/mol) in the tablet: Mass of tablet dissolved in 250.0 mL: 5.422 g Aliquot volume of sample titrated: 25.00 mL Concentration of KIO3: 0.023 M Final burrette volume: 41.31 mL Initial burrette volume: 8.89 mL Blank volume: 0.14 mL
- ) 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=-12Calculate the average activity coefficient of KNO3 in a solution of 0.004 M KNO3 and 0.076 M NaCl.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?