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The solubility of magnesium phosphate at a given temperature is 0.936 g/100 mL. Calculate the Ksp at this temperature.
Express your answers using two significant figures. Enter your answers numerically separated by commas. [HCO2H], [HCO?2], [H3O+], [OH?] = Part C Also calculate the percent dissociation. Express your answer using two significant figures.
When 2 moles of Mg3N2 are allowed to react with water to form ammonia gas and magnesium oxide, how many moles of H2O are required?
A transition mutation for the second codon of glu would result in a gly. Explain the consequences of this, if the glu that was mutated was in the central region of a alpha-helix
Consider the halide ions as nucleophiles. Briefly explain why F-, the strongest base among the halide ions, is the best nucleophile in polar aprotic solvents while iodide the weakest base
Super-green is an indicator with a Ka of 1.6 × 10-7. The acid form is yellow and the base form is blue. Awesome-orange is an indicator with a Ka of 5.0 × 10-5.
At 1000 deg. K, a sample of pure NO2 gas decomposes. 2NO2(g)f/r2NO(g) + O2(g) The equilibrium constant Kp is 158. analysis shows that the partial pressure of O2 is 0.14 atm at equilibrium.
Solid lithium metal and diatomic nitrogen gas react spontaneously to form a solid product. Give the balanced chemical equation (including phases) that describes this reaction.
Calculate the pH of the solution that results when 100.0 mL of 0.15 M NaOH is added to 50.0 mL of 0.25 M HNO3
How many grams of KHP are needed to neutralize 54.63 mL of a 0.1051 M NaOH solution?
Iodide ion catalyzes the decomposition of hydrogen peroxide. the reaction is first-order in H2O2. what is the value of the rate constant,k, if the initial rate is 0.00842 mol/(L*s)?
Calculate the mass of one oxygen atom and determine the number of oxygen atoms in a 10.00g sample of the element.
determine the net change of oxidation number of each of the elements in the redox equations.
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