If 1.25 g of sodium carbonate was dissolved in water and the solution titrated with 22.7 ml of hydrochloric acid to a medal orange end point, calculate (i) the molarity and (ii) the percent by mass (density of sution = 1.02 g/ml) of the hydrochloric acid solution
Calculate the molar concentration of each of the following:
a. 6.0 N sulfuric acid (in reactions that replace both hydrogens)
b. 3.5 N potassium hydroxide
c. 4.0 N phosphoric acid (in reactions that replace two hydrogen ions)
d. 6.2 N sodium hydroxide
1. Consider a buffer solution containing an acid with a pKa of 2.3 and an acid concentration that is one-fourth the concentration of the conjugate base. What is the pH of the solution?
2. Calculate the pH of a buffer containing 0.1 M sodium acetate and 0.2 M acetic acid (pKa= 4.76).
3. The pH of the given solution of lactic acid and lactate is 4.30. Calculate the pKa of lactic acid, when the concentration of lactic acid and lactate are 0.020 M and 0.073 M respectively.
it requires 2 sticks of butter to make a batch of 20 cookies. How much butter will it take to make 150 cookies.
Balance the following reactions by half-reaction method. Identify the oxidizing agent and the reducing agent. Show your process in balancing the reactions.
O.A. R.A.
a. Fe3+ + Sn2+ Fe2+ + Sn4+
b. NO3- + Cu NO2 + Cu2+
I am stuck with how to get half equiv point. I just need help with one demonstration of how to get Veq/2. There were 3 trials, I was able to calculate that Trial 1 had: Mass sample, g= 0.5001
Veq (from 2nd derivative), mL = 13.595
% purity = 57.9
Average % purity of 3 trials = 58.9
and the closest volume and pH is: Trial 1: 14ml, 9.88 pH
1.Given the K values at 25°C, predict the extent of each reaction by indicating whether it is reactant-favored or product-favoured.
N2(g) + 3H2(g)2NH3(g)
K=3.5 ×10^8
CaCO3(s) Ca^+2(aq) + CO3 ^-2, (aq)
K= 3.8 x 10^-9
S(s) + 02(g) ----><------SO2(g)
K=4.2×10^52
AgCl(s) Ag^+1(aq) + Cl^-1(aq)
K=10^-10
It is desired to prepare cupric sulfate solution by dissolving 250 grams of cupric sulfate inenough water to a volume of 900 mL. The solution has a density of 1.405 g/mL. Calculate: a) % by weight of solute c) mole fraction of solute b) Molality d) Normality
The density of toluene, C7H8, is 0.867 g/mL and the density of thiopene, C4H4S , is 1.065 g/mL. A solution is prepared by dissolving 14.0 mL of thiopene, in 250 mL toluene. What is the concentration of thiopene in this solution expressed in:
a. vol %
b. mole %
c. Molarity
d. Molality
Whatever the solvent used, the solution should be topped-up to its final volume using water. True or False?