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The empirical formula of a solid is AB2 and it dissolves to form the cation A2+ and the monoanion B-.
Solid AB2 is added to water and allowed to reach equilibrium. At equilibrium, the concentration of A2+ is found to be 0.24 moles/L. What is the Ksp of this salt?
When an acid or a base is added to a buffer, a double-displacement reaction will occur. The acid or base will be neutralized, forming a neutral salt or water plus the conjugate of the buffer.
what compounds would you use and how would testing these two compounds contribute in your knowledge of the above mentioned subjects
The neutralization of 50.0 mL of 1.00 M hydrochloric acid with 50.0 mL of 1.00 M sodium hydroxide causes a 6.7°C increase in temperature. Predict how the following changes to the experimental protocol would affect the value of the change in temper..
Balance the following equation by the half-reaction method for the pH conditions specified: H2CO (aq) + Ag(NH3)2+ (aq) ? HCO3- (aq) + Ag (s) + NH3 (aq) (basic)
how many grams of calcium hydroxide will be needed to react with 10.0g of phosphate acid(h3PO4). how many grams of calcium phosphate will form?
If 18.5 mL of 0.800 M HCl solution are needed to neutralize 5.00 mL of a household ammonia solution, what is the molar concentration of the ammonia.
You transfer a gas at 25oC from a volume of 2.49 L and 0.950 atm to a vessel at 32oC which has a volume of 8.75 L. What is the new pressure of the gas
Write the molecular, ionic, and net ionic equations for the combination of KNO3(aq) and BaCl2(aq)
307g of an unknown mineral is heated to 98.7 C and placed into a calorimeter that contains 72.4 g of water at 23.6C. the heat capacity of the empty calorimeter was 15.7 J/K. the final temperature of the calorimeter is 32.4C. What is the specific h..
If you have 100mL of 0.1 M acetic acid, pKa 4.7. How much 0.2 M NaOH solution would be needed to fully neutralize the acetic acid
What is the wavelength of the most energetic photons produced by an X-ray tube using U = 24.3 kV potential difference
Ammonia is made industrially by reacting nitrogen and hydrogen under pressure, at high temperature, and in the presence of a catalyst. The equation is N2(g)+3H2(g)---->2NH3(g). If 4.0mol of H2 react, how many moles of NH3 will be produced.
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