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Write a balanced net ionic equation to show why the solubility ofCr(OH)3(s) (Ksp =6.7E-31) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid.
How many grams of CuCl2 are required to prepare 1220. g of a 1.65% (by mass) CuCl2 solution?
In which of the following organ does both physical and enzymatic digestion of lipids occur
a 1.00 liter solution contains 1.00 mol of weak acid HX. After 0.60 mol of Oh- is added to this olution, the pH of the solution is 4.00. Calculate the Ka for the acid HX.
What is the mass (in grams) of the precipitate when 7.1 g of iron(III) chloride reacts in solution with excess sodium phosphate
Starting with a sample of (R)-2,3-dimethylhexan-3-ol, provide the best synthesis of (R)-3-chloro-2,3-dimethylhexane
At 22 °C an excess amount of a generic metal hydroxide M(OH)2, is mixed with pure water. The resulting equilibrium solution has a pH of 11.05. What is the Ksp of the salt at 22 °C
I dont understand how 'n' in the equation turned into 4.35x10^2...where did that number come from
A sample of gold weighs 1.2 oz. The sample is pounded into a thin rectangular sheet with an area of 400. sq. ft. The density of gold is 19.3 grams per cm3. What is the thickness of the foil in centimeters
State an expression for the concentration of a spiked sample (X) if the 5mL of sample with analyte concentration = C was spiked with 2mL of a standard with a concentration of 25.00ppm as well as the whole thing diluted to a total volume of 10.00mL..
there are some given substances likenbsp kohnabr crpo4 rbcl pboh2 lino3nbspnbsp you just need to find out which
the decomposition of hypothetical compound X from part A is 1.60 M -1 * min -1, calculate the concentration of X after 16.0 min. Initial concentration is o.467
What mass of MgNH4PO4 precipitated when 200.0ml of a 1.000% (w/v) solution of MgCl2 were treated with 40.0ml of 0.1753 Na2PO4 and an excess reagent of NH4+
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