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Important information about Quantitative Analysis Problem
Weak acid/Weak Base
1. Calculate the [H3O+], pH, and the fraction of dissociation (α) in an aqueous 0.140 M NH3 solution. (Hint: You will need the Ka, located in the back of your textbook.)
NH3 + H2O ↔ NH4+ + OH-
2. BHClO4 (0.10M) salt is formed from base B (Kb=1.5×10-4) and perchloric acid which dissociated into BH+ (weak acid) and ClO4- (neutral).Find the concentrations for all species in solution, pH, and fraction of dissociation (α).
B + HClO4 → BHClO4 ↔ BH+ + ClO4-
What is the molality of a solution that contains 2.93 grams of urea (molar mass = 60.0 g/mol) in 141 grams of benzene.
What is the potassium concentration of a solution formed by combining 50.0 mL of 0.400 M KCl with 50.0 mL of: a) 0.100 M PdCl6, b) 0.800 M PdCl6 , c) water, d) 0.200 M PdCl6 (If The Ksp for K2PdCl6 = 6 x 10^-10)
What is the smallest possible integer coefficient of S in the combined balanced equation and compute the final pressure in the tank if nothing else is altered in the surroundings.
Solubility Constant, Ksp of Reactant, The chemical reaction representing the soluability of AGBr is: AgBr (right and left arrow) Ag^+ +Br^-
Compute the enthalpy change, , for this reaction per mole of (Assume that the specific heat and density of the resulting solution are equal to those of water [4.18 and 1.00 ] )
What are the probable classes of hydrocarbon or hydrocarbon derivative (i.e.: alkane, alkene. ketone. ester. organic halide, etc...) in each of the following
14.0 moles of gas are in a 6.00 L tank at 22.6 C. Calculate the difference in pressure between methane and an ideal gas under these conditions.
Organic chemistry mechanism and conceptual problems involving, 1. Write equations to show how nitronium ions might be formed using a mixture of nitric and sulfuric acids.
Determine the mass of CuSO4 · 5H2O that must be used to prepare 250 mL of 0.88 M CuSO4(aq).Answer in units of g.
An equilibrium mixture of SO2,O2 and SO3 gases at 1500k is determined to consist of 0.244 mol/L SO2, 0.172 mol/L O2 and 0.56 mol/L SO3.
Hydrogen cyanide is prepared from ammonia (NH3) and natural gas (CH4).2 NH3 (g) + 3 O2 (g) + 2 CH4 (g) → 2 HCN (g) + 6 H2O (g)
0.75g of hydrogen chloride is dissolved in water to make 2.5L of solution. What is the pH of the resulting hydrochloric acid solution.
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