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Problem- Consider the titration of 25mL of 0.1M I- with 0.05M Ag+, where we monitor the Ag+ concentration with an electrode. Determine the pAg after the addition of 10mL of titrant, at the equivalence point, and after the addition of 52mL of titrant. Show the ICE table for each step.
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Calculate the mass (grams) of KHP needed to react with 40. mL of 0.10 M NaOH. B. If 0.7528 g of KHP standard were titrated with NaOH and the endpoint was reached at 36.33 mL
Calculate the [OH-] in 0.050 M potassium fluoride, KF The answer choices are: A. 8.3 × 10-7 M B. 4.7 × 10-7 M C. 6.2 × 10-7 M D. 1.4 × 10-6 M E. 2.2 × 10-6 M
The initial temperature of the calorimeter is 23.0}C. If 7.20g of CaCl2 is added to the calorimeter, what will be the final temperature of the solution in the calorimeter? The heat of solution\Delta H_soln of CaCl2 is -82.8 kJ/mol.
A gas expands from 282 mL to 971 mL at constant temperature. Calculate the work done (in joules) by the gas if it expands against a vacuum.
Which has the lower concentration of hydrogen ions, vinegar at pH 3 or tomato juice at pH 4? How many times fewer hydrogen ions? Which is more acidic?
Problem- Calculate the cell voltage using the following half - reactions, standard reduction potentials and Ksp values for AgCl and PbF2 The concentrations of NaF and KCl are .10M in each half cell
A NaOH solution that is 18.1M, has a density of 1.250 g/ml. What is the molality? Mass Percent? and Mole Fraction?
the vapor pressure of a solution containing 53.6 g glycerin c3h8o3 in 133.7 g ethanol c2h5oh is 113 torr at
Calculate the change in pH across the membrane that is required at 25C to synthesize one mole of ATP from ADP and Pi under standard state conditions. ?rG'=31.4kJ for the synthesis of 1 mole of ATP (mitochondrial ??=-0.15V)
The solubility of suberic acid is 0.14 g/100 ml of water or 0.56 g/100 ml of ether. Calculate the volume of ether needed to remove 90% of the suberic acid from 100 mL of saturated aqueous solution in a single extraction.
A phosphate buffer solution contains 0.08 M K2HPO4 and 0.12 M KH2PO4. PKa values for H3PO4 are 2, 6.8, and 12.2. Compute the concentrations of
What is the pH of a 0.3656 M solution of the sodium salt of a weak acid with a pKa of 3.745? The answer is not pH = pKa + log(salt)
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