1. 5.00 L of a 0.400 M KCl solution
2. 50.0 mL of a 4.00 M HCl solution

50.0 mL of a 0.250 M AgNO3 solution and 50.0 mL of 0.400 M Na2CO3 solution are mixed. How much of the silver carbonate precipitate will be formed? 2 AgNO3 (aq) + Na2CO3 (aq) -> Ag2CO3 (s) + 2 NaNO3 (aq)
To prepare 100 ml of a 50.0 mM solution of KCl from a stock solution that is 1.00 M, use: ___________ ml of 1.00 M KCl and _____________ ml of distilled water The answer: (5.00 ml of 1.00 M KCl and 95.0 ml of water.) But how did they get this answer?
When 50.0 mL of 0.400 M hydrochloric acid and 50.0 mL of 0.200 M calcium hydroxide are combined, the pH of the resulting solution will be : A. Less than 7 B. Equal to 7 C. Greater than 7
Calculate the molarity of each of the following: a. 2.00 mol of glucose in 4.00 L of a glucose solution b. 4.00 g of KOH in 2.00 L of a KOH solution c. 5.85 g of NaCl in 400. mL of a NaCl solution Calculate the grams of solute needed to prepare each of the following: a. 2.00 L of a 1.50 M NaOH solution b. 4.00 L of a 0.200 M KCl solution c. 25.0 mL of a 6.00...
50.0 50.0 mL solution of 0.113 0.113 M KOH KOH is titrated with 0.226 0.226 M HCl HCl . Calculate the pH of the solution after the addition of each of the given amounts of HCl HCl . 0.00 mLpH= 0.00 mLpH= 5.00 mLpH= 5.00 mLpH= 12.5 mLpH= 12.5 mLpH= 19.0 mLpH= 19.0 mLpH= 24.0 mLpH= 24.0 mLpH= 25.0 mLpH= 25.0 mLpH= 26.0 mLpH= 26.0 mLpH= 29.0 mLpH= 29.0 mLpH=
100.0 mL of 3.00 M HCl (in water) is added to 50.0 mL of 5.00 M NaOH in a beaker. What is present in the beaker?
Assume that 100.0 mL of 0.200 M CsOH and 50.0 mL of 0.400 M HCl are mixed in a calorimeter. The solutions start out at 22.50 ∘C, and the final temperature after reaction is 24.28 ∘C. The densities of the solutions are all 1.00 g/mL, and the specific heat of the mixture is 4.2J/(g⋅∘C). Calculate the energy which releases in the process. Express your answer using four significant figures.
A 50.0 mL solution of 0.160 M KOH is titrated with 0.320 M HCl. Calculate the pH of the solution after the addition of each of the given amounts of HCl. 0.00 mL pH = 5.00 mL pH = 12.5 mL pH = 19.0 mL pH = 24.0 mL pH = 25.0 mL pH = 26.0 mL pH = 29.0 mL pH =
When 100.0 mL of 0.200 M CsOH is added to 50.0 mL of 0.400 M HCl in a coffee cup calorimeter at 22.50 degree celsius, the temperature rises to 24.28 degree celsius. Calculate the Delta-H of this reaction per mole of CsOH (assume total volume is sum of two volumes, density of the mixed soln is 1.00 g/mL & the specific heat of the soln is 4.2 J/g-K)
A 0.400 g sample of KCl(s) is added to 50.0 g of water in a calorimeter. If the temperature decreases by 0.95˚C, what is the approximate amount of heat involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g˚C?