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Calculating the concentration of the acetate ion when dissociation of acetic acid occurs in water and over varying pH conditions?I am a process engineer in wood pulping operation in which we use steam to digest hardwood chips. This is non-chemical pulping, but the residual "wood juice" for lack of a better term has a pH as low as 3.0 and contains significant concentrations of acetic acid.
Now consider that acetic acid in a water solution in which the pH is 3.0. Assume more water is added to the solution so that via dilution the pH increases to 4.5, and then again to 6.5.
How would I calculate the change in the acetate ion concentration at pH 3.0, 4.5, and 6.5?
I know the acetate ion would have a strong attraction to cations in the water solution such as Na, Ca, and Zn if present....would you think that the presence of the acetate ion would inhibit downstream ionic bonding of highly anioinc resins and waxes that we put in the wood pulp after steaming?
PCl5 + 4H2O > 5HCl +H3PO4. How many total moles of acid are formed when starting with 4.5 g of PCl5 and excess H2O.
Some of the cyclohexane solvent vaporized during the temperature versus time measurement. Will this loss of cyclohexane result in its freezing point being recorded as too high, too low, or unaffected.
Calculate what quantity of potassium chlorate that has molecular weight of 122.5 needed to form 33.6 litres of oxygen? Express your answer in grams and assume that temperature and pressue will be in normal condition?
How much CH4, in grams, is needed to produce 50.0 grams of CHCl3?
An empty gasoline can with dimensions 15 cm by 40 cm by 12.5 cm is attached to a vacuum pump and evacuated. if the atmospheric pressure is 14.7 lb/in^2.
The half of cesium-137 is 30.2 years. If the initial mass of sample of cesium-137 is 1,000 g, how much cesium will remain after 151 years.
A 25.0 mL sample of a solution of the weak base aniline, C6H5NH2, requires 25.67 mL of 0.175 M HCl to reach the equivalence point. (Kb for aniline = 4.0 x 10-10)
An aqueous solution contains 167 g CuSO4 in 820 mL of solution. Calculate the : a. Molarity b. Percent by mass c. Mole fraction d. Molality of the solution, The density of the solution is 1.195 g/mL
A solution is made by dissolving 0.0350 mol of HF in enough water to make 1.00L of solution. At 24°C, the osmotic pressure of the solution is .975 atm.
What is the formula of the zinc sulfate hydrate? name this compound
C12H22O11(aq) + 3 O2(g) 2 H3C6H5O7(aq) + 3 H2O(l) Determine the mass of citric acid produced when 4.60 mol C12H22O11 is used.
Determine how much heat is formed by this reaction if a typical packet has 250 g of Fe to warm your hands (or feet for up to 4 h) express your answer in kJ?
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