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Write net ionic equations for the following molecular equations. HBr is a strong electrolyte. (Include states-of-matter under SATP conditions in your answer. Use the lowest possible coefficients.)
(a) HBr(aq) + NH3(aq) → NH4Br(aq)(b) 2 HBr(aq) + Ba(OH)2(aq) → 2 H2O(l) + BaBr2(aq)(c) Pb(NO3)2(aq) + 2 NaBr(aq) → PbBr2(s) + 2 NaNO3(aq) (d) MgCO3(s) + H2SO4(aq) → MgSO4(aq) + H2O(l) + CO2(g)
what the oxidation state P in PO4^-2? what the oxidation state O in PO4^-2?
What is the pH of a solution that is 0.75 M in sodium acetate and 0.50M in acetic acid? (Ka for acetic acid is 1.85 x 10-5).
What is the rate law for step 1 of this reaction? ((Express your answer in standard Mastering Chemistry notation.
Balance the equation and determine the mass in grams of chlorine that would be formed if 25 grams of PCl3 (molecular mass = 137.32 g/mol) decompose.
An excess of AgNo3 reacts with 110.5 of an AlCl3 solution to give 0.215g of AgCl. What is the concentration in moles per liter?
Calculate the percent (by volume) of air that would be displaced when all of theN2 (l) get evaporated. it is given that Liquid nitrogen has a density of 0.807 g/mL
The Ka of a monoprotic weak acid is 7.76 × 10-3. What is the percent ionization of a 0.127 M solution of this acid?
By Solving this problem student understand about isotopic abundance and how to calculate atomic weight (average atomic mass) of an element -
A stream of humid air containing 1.00 mole % H2O(v) and the balance dry air is to be humidified to a water content of 10.0 mole % H2O. For this purpose
0.0010 mg of H, 0.0116 mg of C, and 0.0310 mg of O. It was also determined that the unknown compound had a molecular weight of 90.0 g/mol.
How many grams of Cu metal (63.55 g/mol) will be plated out of a Cu(NO3)2 solution by passing a current of 3.00 amperes for 11 minutes?
A gas expands and does P-V work on the surroundings equal to 327 J. At the same time, it absorbs 121 J of heat from the surroundings. Calculate the change in energy of the gas.
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