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A solution is prepared by mixing 79.0 mL of 5.00 M HCl and 34.0 mL of 8.00 M HNO3. Water is then added until the final volume is 1.00 L. Calculate [H+ ], [OH - ], and the pH for this solution.
How many grams of solute are required to make a 147 mL solution of sodium hydroxide with a concentration of 0.5330 M.
In a 1.00 L flask, 3.40 atm of CO reacts with 2.60 atm of O2. Assuming that the temperature remains constant, what is the final pressure in the flask.
A gas has a pressure of 4.82035 atm when its volume is 2.75 L. What will the pressure be when the volume is changed to 1.91015 L, assuming constant temperature.
A chemist wishes to prepare 200mL of a saturated solution of BaF2, the concentration of which is 6.3 x 10-3 mol/L. Determine the mass of BaF2 that will be needed to make up the 200mL of the solution.
mixture(O,H) is ignited with a spark and it reacts to form (H2O)liquid water. determine the temperature of water.
Calculate the initial rate of the NO reduction at 1100 K if 400.00 mg of NO and 600.00 mg of H2 are confined to a 5.00 L reaction vessel.
how many grams of NO are required to produce 145 g of N2 in the following reaction? 4NH3+6NO-- 5N2+6H2O
Calculate the molar concentration of OH - ions in an 1.43 M solution of hypobromite ion, BrO- (Kb = 4.0 10-6).
Determine the pressure in a 14.6 L cylinder filled with 0.440mol of N2 gas at a temperature of 327K.
If 1.50 g of (NH4)2SO4 is dissolved in enough water to form 200. mL of solution, what is the molarity of the solution.
Write a balanced nuclear equation for the alpha decay of each of the following radioactive isotopes.
What is the percentage yield of SO3 if 22.3 g SO3 are obtained from the reaction of 25.0 g SO2 with an excess of O2.
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