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Calcium hydrogen phosphate is a component of plant fertilizers (a source of phosphate). It is a relatively insoluble hydrated ionic compound, CaHPO4·2H2O, with a Ksp of 2.7×10-7 at 25°C
a) Write a balanced equation describing a saturated solution of CaHPO4·2H2O, and write the Ksp expression.
b) "Hard" water contains relatively high concentrations of dissolved calcium ions. Calculate the solubility (in molarity) of CaHPO4·2H2O at 25°C in hard water that initially contains 95 mg/L of Ca2+
c) Imagine you will add this fertilizer solution to soil (earth) that is acidic, because there are pine trees growing in the area. How will the low pH affect the solubility equilibrium of CaHPO4·2H2O? Name the "effect" involved?
how many grams of khp are needed to exactly neutralize 27.4 ml of a 0.235 m potassium hydroxide
Show your calculations for the pH when 0.00 mL, 4.00 mL, 6.00 mL, 12.00 mL (equivalence point), and 16.00 mL of 0.10 M HCl have been aded to an initial
Determine the % relative error for the following quantities: if there is no uncertainty given for a specific value, assume an absolute error of "1" in the last digit.
Asprin, whose structure can be found in the introduction, can be made from the reaction of a phenol and an anhydride. Give the phenol and anhydride that could be used to make aspirin?
What is the percentage yield if 465 grams of hydrogen reacted with excess nitrogen and 455 grams of ammonia is formed N2 (g) + 3 H2 (g) 2NH3(g)
At 1478 oC the equilibrium constant for the reaction: 2 IBr(g) ? I2(g) + Br2(g) is KP = 0.899. If the initial pressure of IBr is 0.00169 atm, what are the equilibrium partial pressures of IBr, I2, and Br2? p(IBr) = . p(I2) = . p(Br2) = .
What will be the products of the electrolysis of an aqueous solution of silver fluoride (AgF). (The electrodes themselves are platinum.)
The energy from condensing steam water is used to melt ice at 0 degrees Celsius. How much ice can be melted by condensing 1.0 kg of H2O vapor? (Delta H fus of ice= 6.01 kj/mol) (Delta H vap of water = 40.7 kj/mol)
Suppose that 1.252 g of impure barium hydroxide is dissolved in enough water to pro- duce 213.4 mL of solution and that 64.3 mL of this solution is titrated to the stoichiometric point with 29.5 mL of 0.0318 M HCl(aq). What is the percentage purit..
When heated, ammonium carbonate decomposes as follows. NH4CO2NH2(s) ->2 NH3(g) + CO2(g) At a certain temperature the equilibrium pressure of the system is 0.318 atm. Calculate KP for the reaction.
Liquids cannot be compressed easily. What does this imply about the amount of space that must be present between the individual liquid particles?
A cobalt compound has an observed magnetic moment of 5.2 B.M. What can you deduce about the compound?
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