The ionization constant of a very weak acid, HA, is 5.8×10-9. Calculate the equilibrium concentrations of H20", A", and HA in a 0.040 M solution of the acid. Determine the concentrations of all species at equilibrium and the solution pH. [H;O"]=| mol/L [A]=| mol/L [HA] = mol/L %3D pH =
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- A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?Calculate the volume (ml)of concentrated ammonia and the weight (gm) of ammonium chloride respectively to be taken to prepare 100 ml of buffer solution at a pH of 10 if the final concentration of the salt is 0.20 mol. Note that the molar concentration of concentrated ammonia is equal to 14.8 mol/liter, and that the pKb of ammonia is 4.76, and the molecular weight of ammonium :chloride 53.5 g/mole.lt is about1. a. A 250.0ml of a solution of the strong base, CsOH(MW = 150.0 g/mole) is made. The pH is measured to be 8.90. What mass of cesium hydroxide is present in the solution? b. The surface of Venus is quite inhospitable with an average temperature of 450 ̊C and a pressure of 92 atm (earth). Under these delightful conditions, the pKw of water is estimated to be 24. What is the pH of neutral water on Venus? c. An aqueous acetic acid (HOAc) solution is 1.00 % dissociated. What will the concentration of H3O+ be if 0.82 g of sodium acetate (NaO2C2H3) is added to 100.mL of solution? d. PICTURE ATTACHED Glutaric Acid is a diprotic organic acid with a molecular formula of H2C5H6O4, and a molecular weight of 132.12 g/mol. The stepwise acid dissociation reactions and the Ka values are given below. An aqueous solution is prepared by dissolving 1.02 g of glutaric acid in water to form 500.0 ml of solution. Calculate the pH, [H2C5H6O4], [HC5H6O4–], and[C5H6O42–] after the solution has reached…
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