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Calculate the pH of 1.00 L of the buffer 1.01M CH3COONa/1.01M Ch3COOH before and after the addition of the following species. (Assume there is no change in volume). (a) pH of starting buffer: (b) pH after addition of 0.075mol NaOH: (c) pH after further addition of 0.119 mol HCl
The solution to Equilibrium constant, A certain gas mixture held at 395C has the following initial partial pressures: P(Cl2) = 351.4 torr; P(CO) = 342.0 torr and P(COCl2) = 0.
If 323 g of magnesium reacts with excess oxygen to produce 296 g of magnesium oxide, what is the percent yield for the reaction?
If 1.50g (NH4)2SO4 is dissolved in enough water to form 250 ml of solution, what is the molarity of the solution.
CaH2(s) + 2H2O(l) Ca(OH)2(aq) + 2H2(g) How many grams of CaH2 (Molar Mass = 42.1 g/mol)are needed to generate 10.0 L of H2 gas if the pressure of H2 is 769 torr at 28.0°C?
A student carefully diluted 25.0mL of 6M NaOH solution in 475mL of distilled water. Calculate the molarity of the diluted solution of base.
How many grams of dry NH4Cl need to be added to 2.50 L of a 0.500 it M solution of ammonia, NH3, to prepare a buffer solution that has a rm pH of 8.99?
2 FeS + 3 N2 → 2 FeN + 2 SN2 This reaction has a 65.0% yield. How much N2 is consumed if 13.6 g of FeN are produced?
Determine how do you find out the new freezing point of a solution if given the formula is Delta T = m x kf x i but how do you find it how does it work?
A graduated cylinder contains 131 mL of water. A 18.0 g piece of iron (density = 7.86 rm{g/cm^3}) and a 25.0 g piece of lead are added.
what is the correct electron configuration for Cr (chromium). Chose the proper Lewis dot structure for the compound or poliatomic ion: Sulfur Dioxide (SO2).
61.5 mL of 0.11 M sodium hydroxide were required to completely neutralize 23.7 mL of sulfuric acid. Calculate the concentration of the sulfuric acid solution
A sample of water in the vapor phase (no liquid present) in a flask of constant volume exerts a pressure of 429 mm Hg at 97 °C. The flask is slowly cooled
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