1. If the potassium hydrogen phthalate is not completely dry, how would it affect the reported molar concentration (molarity) of the NaOH solution in Part A? Explain. 2. In Part A, the mass of KHC;H4O4 is measured to the nearest 0.0001 g. However, the volume of water used to dissolve the KHP does not need to be precise. Explain why the amount of water added to KHP has no effect on the experimental results. 3. Identify two possible sources of experimental error in this experiment, and describe the effect of each error in the determination of the molar concentration (molarity) of the acid solution in Part B.

1. If the potassium hydrogen phthalate is not completely dry, how would it affect the reported molar concentration (molarity) of the NaOH solution in Part A? Explain. 2. In Part A, the mass of KHC;H4O4 is measured to the nearest 0.0001 g. However, the volume of water used to dissolve the KHP does not need to be precise. Explain why the amount of water added to KHP has no effect on the experimental results. 3. Identify two possible sources of experimental error in this experiment, and describe the effect of each error in the determination of the molar concentration (molarity) of the acid solution in Part B.

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Chapter17: Solubility And Complex-ion Equilibria

Section: Chapter Questions

Problem 17.112QP

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has abr 9. What is the molarity of a solution that contains 2.38 g of H₂C₂O4 2H₂O in exactly 300 mL of solution? ont ut 10. If 25.21 mL of NaOH solution is required to react completely with 0.550 g KHP, what is the molarity of the NaOH solution? 11. The titration of an impure sample of KHP found that 36.00 mL of 0.100 M NaOH was required to react completely with 0.758 g of sample. What is the percentage of KHP in this sample? 12. How many milliliters of 0.250 M NaOH are required to neutralize 30.4 mL of 0.146 M HC1?
A 50.00-mL sample of white wine required 24.57 mL of 0.03291M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL. (Assume that two hydrogens of the acid are titrated.)
15
9. We prepared a solution containing 1.0 mol.L' HF and 1.0 mol.L·' C,H3OH. The K, of hydrofluoric acid and phenol are 7.2 x 104 and 1.6 x 10-10 respectively. What is the pH of this solution? (Hint: find which acid is strongest and make the appropriate assumptions) b. What is the concentration of C,H;O¯ at equilibrium? а.
11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting the resulting solution to a volume of 1.0 L. What is the effect of adding 0.020 mol CH3COO (aq) to this solution? How will pH change (calculate pH before and after the addition. Ka of CH3COOH is 1.76 x10-5)? How will concentrations of CH3COOH and CH3COO at equilibrium change?
5:50 1 Search Question 5 of 20 Submit Determine the mass of solid NaCH;COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH3COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH-COОH is 1.8 х 10-5. 1 2 Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH3COOH+ H20(1) =H;O*(aq) +CH3COO-(a Initial (M) Change (M) Equilibrium (M) 5 RESET 0.200 5.00 -5.00 1.0 x 10-9 -1.0 × 10-9 1.0 x 10-5 -1.0 x 10-5 1.8 x 10-5 -1.8 x 10-5 х+ 5.00 x - 5.00 x + 1.0 × 10-9 х - 1.0 х 10-9 1.0 x 10-5 x - 1.0 × 10-5 x + 1.8 × 10-5 х - 1.8 х 10-5
An intrinsic property is one a That is dependent on how much of the material is present That is analogous to the flammability of any substance That is analogous to the flammability of any substance That only changes withaltitude How many moles are in 20 mg of steric acid, CH_3(CH_2)_{16}COOH?
What are the molar concentrations of acetic acid (CH3COOH) and sodium acetate (CH3COONa) in an aqueous solution buffered at a pH of 4.22 that has a freezing point of −2.87 °C? Assume complete dissociation of sodium acetate and a density of 1.02 g/mL for the solution. The p?a for CH3COOH is 4.75.
The 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.
6. A buffer solution is formed by adding 0.500 mol of sodium acetate (CH3CO2NA) and 0.500 mol of acetic acid (CH3CO2H) to 1.00 L H,0. What is the pH of the solution at equilibrium? (K, = %3D 1.8 x 10°)
19.80 mL NaOH is required to titrate 0.6013 g of potassium hydrogen phthalate (KHC8H4O4). How many mL NaOH required to titrate 25.0 mL 0.10 M HCL solution?
Give a list of laboratory apparatus and equipment that are to be utilized for the preparation of 100 mL of 5 M NH 3 Cl.

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