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Q1. Using the ICE table Calculate the pH of a solution that contains 0.0075 M Lactic acid and 0.085 M sodium lactate.Q2. Use the Henderson equation to calculate the pH of the buffer solution in Question 1. Compare your answer to the one obtained from Q1.Q3. What combination of substances will give a buffered solution that has a pH of about 8? Explain the reason for your choice. NH3 mixed with NH4Cl (Kb for NH3 = 1.8 x10-5) or C5H5N mixed with C5H5NHCl (Kb for C5H5N = 1.7x10-9)Q4. Calculate the pH of a solution that is 0.210 M in Methylamine and 0.350 M in Methylamine hydrochloride.Q5. Calculate the pH of a buffer prepared by mixing 50.0 mL of 1.00 M ammonia and 50.0 mL of 1.00 M ammonium nitrate (Remember to take dilution into account)Q6. A solution contains 0.37 moles Formic acid (Ka= 1.77 x10-4) and 0.23 moles Sodium formate in 1.0 L of solution.a) Calculate the pH of this solutionb) What will be the pH of the solution after 0.15 mol of NaOH(s) is added to the buffer in (a)c) What will be the pH of the solution after 0.15 mol of HCl(g) is added to the buffer in (a)Q7. 25.0 ml of 0.723 M HClO4 is titrated with 0.273 M KOH. Calculate the pH of the HCl solution at each of the following steps in the titration.a) Initially before any KOH has been added.b) 10.0 ml of KOH has been addedc) 25.0 ml of KOH has been addedd) At the equivalence point.e) 70.0 ml of KOH has been addedQ8. Our blood buffer system includes a combination of H2CO3 with HCO3-. If Ka1 (H2CO3) = 4.3x10-7, what is the ratio of [HCO3-]/ [H2CO3] needed to maintain a pH of 7.40?Q9. Consider the titration of 25.0 mL of 0.200 M NH3 (Kb = 1.8 x 10-5) with 0.200 M HCl. a) What is the initial pH of the NH3(aq)? b) What is the pH halfway to the equivalence point? c) What is the pH at the equivalence point? d) Sketch the titration curve. Label the point(s) where there is a A) a weak base B) weak acid C) Buffer D) Strong acid in excess,Q10. The solubility of Ag2SO4 is found to be 4.5 g/L.a) Calculate the molar solubility of Ag2SO4.b) What is the Ksp for Ag2SO4?Q11. What is the molar solubility of PbCl2 in 0.15 M HCl (Ksp for PbCl2 = 1.17 x 10-5)Q12. The Ksp of Zn(OH)2 is 5.0 x 10-17. Calculate the concentration of the Zn2+ ions in a solution of Zn(OH)2 that has a pH of 9.62.Q13. The Ksp of BaF2 is 2.45 x 10-5. a) Calculate its Molar solubility. b) What is the solubility in grams per liter.Q14. Is CaF2 is more soluble in a solution of pH = 2 or pH = 9? Explain the reason for your answer clearly.
How much heat do you need to raise the temperature of 150 g of gasoline from 30oC to 15oC?
A 31.43 ml volume of .108M NaOH is require to reach the phenolphthalein endpoint in the titration of a 4.441g sample of vinegar. Calcute the percent acetic acid in the vinegar.
Suppose you have made 1L worth of a mixture of methanol and water, by mixing 3 parts of methanol and 2 parts of water by mass. Assume for simplicity that the volume of the mixture is exactly equal to the sum of the volumes of the ingredients (whic..
Which of the following is the most effective buffer system for a pH value of 4.45?
consider a particle in a one-dimensional box of length l in its lowest energy ground stationary state. calculate the
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when 100 ml of an aqueous solution containing 1.0 g of caffeine is extracted with 10 ml of chloroform at room
Concentrated hydrochloric acid solution contains 37.2 m/m% HCl. What mass of HCl is contained in 35.5g of concentrated HCl
Molecular formula of C10H14. The carbon NMR shows 7 carbon peaks and 4 H peaks. H(4) broad multiplet at 7.0, H(3) singlet at 1.4, H(1) multiplet at 1.2, and H(6) doublet at 1.0. Has strong UV absorbance at 260nm
determine the specific heat capacity of a metal that has a mas of 14 grams. As the metal cools from 400 degrees celcius to 200 degrees celcius, 364 joules of heat is released
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