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What is the numerical value of the activity coefficient of aqueous ammonia (NH3) at an ionic strength of 0.7?
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- Distinguish between the terms slightly soluble and weak. electrolyte.The pH factor is a measure of the acidity and alkalinity of water. A reading of 7.0 is neutral; values in excess of 7.0 indicate alkalinity; those below 7.0 imply acidity. In one study, it is mentioned that the best chance of catching bass occurs when the pH of the water is in the range 7.5 to 7.9. Suppose your suspect that acid rain is lowering the pH of your favourite fishing spot and you wish to determine whether the pH is less than 7.5. You obtained 10 samples and got the following data: 7.3, 7.4, 7.2, 7.0, 7.5,7.4,7.3,7.3,7.2 and 7.1. Use 0.05 alpha. a. State the alternative and null hypothesis. b. Is the pH of the water samples less than 7.5?Precipitation is the opposite of dissolution. Group of answer choices True False
- 7) An aqueous solution containing 25.0 mg of a hormone in 150.0 mL of solution with an osmotic pressure at 25 °C of 9.00 mmHg. What is the molecular weight of the hormone? 8) (a) What is the pH of a solution in which 45 mL of 0.10 M sodium hydroxide is added to 25mL of 0.15M hydrochloric acid? (b) A brand of carbonated beverage has a pH of 3.50. Calculate [H*]=?6. (i) Define pH in words. The strong acid HClahas a pH value of 1, use the following equation for a strong acid: H+, + and convert the following expression to deduce the hydrogen ion concentration: pH = -log10 [H*] (ii) Use the above expression to deduce the pH of HCL (ag) given the concentration of the acid to be 4.5 mol/dm3 pH =7 (a) Describe what happens when each of the following molecules is separately dissolved in water and illustrate with an equation in each case: (i) ethanoic acid (CH₂COOH) (ii) ammonia (NH3) (b) Identify the conjugate acids and bases in the substances mentioned in question 7(a) above. (c) Explain the difference between: (i) a strong acid and weak acid and (ii) a strong base and a weak base
- 13.3) A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 185 mL of a solution with the same pH? Kb (CN–) = 1.7 × 10–5Three acids found in foods are lactic acid, LA, (in milk products), oxalic acid, OA, (in rhubarb), and malic acid, MA (in apples). The pKa values are LA =3.88, OA =1.23, and MA =3.40. Which list has the conjugate bases of these acids, lactate, oxalate, and malate, in order of decreasing strength? O lactate > malate > oxalate lactate > oxalate > malate malate > lactate > oxalate oxalate > malate > lactateCalculate the analytical concentration of a 1:1 dilution of concentrated ammonium hydroxide? Mixture of 1 part ammonia, to one part water
- A 0.495 M solution of a weak base has a pH of 11.00. What is the base hydrolysis constant, Kp, for the weak base? K, =A 0.018 M solution of salicylic acid, HOC6H4CO2H, has the same pH as 0.0038 M HNO3solution. (a) Write an equation for the ionization of salicylic acid in aqueous solution. (Assume only the –CO2H portion of the molecule ionizes.) (b) What is the pH of solution containing 0.018 M salicylic acid? (c) Calculate the Ka of salicylic acid.A chemical system is set up by placing some solid ammonium chloride in an ammonia solution. The equilibrium established can be represented as follows: NH4*(aq) + H2O(e) 2 H30*(aq) + NH3(aq) The pH of the solution is taken, then a small amount of NaOH(aq) is added and the pH is taken again. What can be said about the change in pH for the solution? The pH significantly increases because a strong base has been added to the solution. The pH significantly decreases because a strong base has been added to the solution. There is very little change to the pH of the solution. If anything the pH of the solution decreases slightly. There is very little change to the pH of the solution. If anything the pH of the solution increases slightly.
