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For each of the following pairs of ions, determine whether a precipitate would form when solutions containing these ions are mixed and write the formulas of any precipitates that should form. Indicate the color of any precipitate that should form.
a. Na+ and I^- b. Ba^2+ and SO4^2- c. Pb^2+ and NO3^1 d. Ag^+ and S^2-
If 315 ml of hydrogen gas is collected over water at 25 degrees C at a total pressure of 742 mm Hg , how many grams of Zn reacted?
The following ions contain the same number of electrons. Rank them in order of decreasing ionic radii.
If a solution contains 0.60 mol of OH^-, how many moles of H^+ would be required to reach the equivalence point in a titration. Express your answer using two significant figures.
What volume of 3.00M HCL in liters is needed to react completely (with nothing left over)
the following compounds has the highest boiling point and which has the lowerst boiling point? explain your answer. a- CH3OCH3 b- CH3COOH c- CH3CH2CH3
A solution is made by combining 10.0 mL of 16.5 M acetic acid with 5.60 g of sodium acetate and diluting to a total volume of 1.50 L. Calculate the pH of the solution.
What is the molar solubility of CaF2 in 0.10 M NaF solution at 25°C? The Ksp for CaF2 is 1.5x10^-10.
Draw a free energy profile for a reaction S to P that proceeds through a single transition state with Delta G knot equal to +2.8 kcal/mol and delta G double dagger equal to 14 kcal per mole. Label the appropiate difference.
What mass of NaHCO3 (M = 84.0) is required to completely neutralize 25 mL of 0.125 M H2SO4? answer is 0.525 g please expline how
Calculate the equilibrium concentrations of I2, Cl2, and ICl. (Kc = 0.110 at this temperature.)
Calculate the pressure of 1.00 mole of CH4 in a 1.00 L container at 300.0 K using first the vand der Waals equation
the Ka of hydrazoic acid (HN3) is 1.9*10^-5 at 25 degrees C. what is the pH of a .35M aqueous solution of HN3?
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