1. (a) Using activities correctly and the short form of the Debye-Hückel model, calculate the pH of a solution initially containing 0.010 F NaOH and 0.0120 F HNO3. (b) What is the pH in the above solution if you neglect activity?
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Show your work, use general chemistry rules for significant figures.
1. (a) Using activities correctly and the short form of the Debye-Hückel model, calculate the pH of a solution initially containing 0.010 F NaOH and 0.0120 F HNO3.
(b) What is the pH in the above solution if you neglect activity?
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- An alkaline sample of sodium compounds weighing 1.196 g was dissolved in water, cooled at 15 deg C, treated with 2 drops of phenolphthalein indicator and titrated with 1.058 N H2SO4 requiring 6.8 mL to render the solution colorless. Upon adding 2 drops of methyl orange and continuing the titration 16.5 mL more of the acid was needed to complete analysis. What is the quantitative composition of the sample?This question concerns the changes which take place when a 0.1M solution of sodium hydroxide is added to 25cm3 of 0.1M hydrochloric acid. In 3 separate experiments, changes in temperature, pH, and electrical conductivity did take place in the cell, respectively. On the axes below, use broken lines(------) to indicate the results you would expect if 0.1M ethanoic acid were used instead of hydrochloric acid. Temperature arbitrary scale against Volume of alkali in cm3 pH against alkali in cm3 Conductivity against alkali in cm3What is meant by the salting out effect? Illustrate.
- The first step in purifying the urine collected on the ISS is to treat every liter of urine with 20 mL of 1.0 M H2SO4. To simplify the calculations, lets assume that urine is water. a) What is the pH of a solution of 20. mL of 1.0 M H2SO4 added to 1.00 L water? To determine this, you can safely assume that 100% of the H2SO4 reacts to form H3O+ and HSO4- ions. Use pKa2 (1.92) to determine if any more protons are added to the solution from HSO4-.In this activity, you will develop an experimental procedure to solve a problem. Consider the followingscenario:You are the manager of a chemical stockroom, and find a bottle containing approximately one liter of aclear and colorless solution of unknown identity and concentration. Your only clue to its identity is thatit was found between bottles of silver fluoride and sodium fluoride, so it is likely an aqueous solution ofone of those two compounds. You will need to develop a procedure to determine the following:a) The identity of the unknown solutionb) The concentration of the unknown solutionWrite out a precise procedure, which includes all glassware, reagents, and steps. You will also need towrite the calculations that you would need to determine the concentration of the solution. Assume thatyou have access to any reagent you might needThe salt K2HPO4 (potassium hydrogen phosphate) is a strong electrolyte but not a strong acid or base. Consider an F = 0.010 M solution of K2HPO4. a) Add the acid/base behavior of hydrogen phosphate by writing a “sequential dissociation scheme” for phosphoric acid (H3PO4). Then write mass balance equations for total phosphate and total potassium and give their numerical values. b) Write the charge balance equation for this solution. How may total species are there? [Count species in the charge balance equation and add any neutrals.] How many additional equations are needed for systematic treatment of equilibrium? Name them (give their usual symbols) c) Consider the KHPO4−(aq) ion pair. This is a new species, so what additional equation would you need? Tell how you would alter each charge or mass balance equation (if necessary) to include this species.
- The acid-dissociation constant at 25.0°C for hypochlorous acid (HClO) is 3.0 × 10-8. At equilibrium, the molarity of H3O+ in a 0.044 M solution of HClO isClearly demonstrate which reactant salt would be limiting if the Experiment1 was performed with solutions of equal concentrations. Assume 20 mL each of 0.5 M solutions, for instance. Show calculations 20 mL 0.5 M BaCl2 solution, and 20 mL of 0.5 M Na3PO4 3BaCl2 (aq) + 2Na3PO4 (aq) ---> Ba3 (PO4)2 (s) + 6NaCl (aq)Do you agree/disagree with the following statement below? State your reasons. "Classical precipitation gravimetric analysis is best used towards the end of quantitative analysis while classical volumetric analysis is best used as the first technique to quantify analytes."
- Determine the pH and concentration of all species at equilibrium for the basic 5-fluorouracil species (C4HFN2O22-). Justify the use of approximations if necessary.Provide the equation for the mass balance of this solution. C4HFN2O22-= 0.30 MSummarize a procedure that will allow you to accurately prepare a series of solutions that are of the following molar concentrations (0.1, 0.05, 0.025, 0.0125, and 0.00625) from 0.200 M stock solution.This question concerns acid-base. Below is a schematic diagram of the apparatus used in measuring PH of a solution. What is the name of the right hand electrode? Give the composition of the calomel electrode. Explain briefly how the set-up works in measuring the PH of a solution.