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1. How many grams of potassium acetate are needed to make the buffer solution? (Ka of acetic acid is 1.78 x 10^ -5)
2. Give the rate expression (rate law) for the following reaction. CO (g) + NO2 (g) -----> CO2 (g) + NO (g)
b) Describe how you would set up an experiment to determine the order of the reaction.
Give the reaction products of sodium borohydride (followed by acidification) with the following compounds. a) acetone
The molecular formula of glycine (an amino acid) is NH2CH2COOH, the molecular mass is 75.07grams/mole. If 10 glycines are joined together by a dehydration reaction to make a polypeptide, what would the molecular mass of the polypeptide equal.
Celcius and add 130.0mL of water at 95.00 Celcius, what is the final temperture of the mixture? Use 1.00 g/mL as the density of water.
we did the grignard reagent experiment and one of the post-lab questions iswhat kinds of solvents cannot be used? give
A solution of 0.0385 M hypochlorous acid, HOCl, has a pH of 4.47. Calculate the acid dissociation constant Ka.
An excess sample of solid Ag2SO3 is added to 100 mL of water. After equilibrium is achieved between the solid and its aqueous ions the silver ion concentration is found to be 2.175e-05 Use this information to find Ksp for Ag2SO3
What are the net ionic equations for: 1. Potassium Fluoride and Ammonium Chloride and 2. Sodium Hydrogen Sulfite and Potassium Cyanide
Provide a structure for the following compound: EI mass spectrum: two molecular ions of about equal intensity at m/z = 180 and 182; IR: 1740 cm-1; 1H NMR: ? 1.30 (3H, t J = 7 Hz); ? 1.80 (3H, d, J = 7 Hz); ? 4.23 (2H, q, J = 7
What is the pressure (in atmospheres) of a sample of gas trapped in the closed-tube mercury manometer
the mineral greenockite is a rare yellow sulfide of cadmium that is 78.0% cadmium and 22.0% sulfur by mass. Determine the empirical formula of greenockite.
if the solubility of a gas is 7.5 gl at 404 kpa pressure what is the solubility of the gas when the pressure is 202
Consider the chemical reaction 2NH3(g) N2(g) + 3H2(g). The equilibrium is to be established in a 1.0 L container at 1,000 K, where Kc = 4.0 ? 10-2. Initially, 1,220 moles of NH3(g) are present. Estimate the equilibrium concentration of H2(g).
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