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A saline solution contains 1.9% NaCl by mass. How much NaCl is present in 83.2 g of this solution?
Chlorine dioxide, ClO2, si a reddish-yellow gas that is soluble in water. In basic solution it gives ClO3- and ClO2- ions. 2ClO2(aq) + 2OH-(aq) ? ClO3-(aq) + ClO2- (aq) + H2O. To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of the reaction of ClO2 as determined. Obtain the rate law and the value of the rate constant.
P4(s) + F2(g) PF3(g) What mass of F2 is needed to produce 151 g of PF3 if the reaction has a 79.3% yield?
Provide the following information for a titration analysis involving a titrant and titrand, where the titrand is a weak, diprotic acid (Ka1 = 1.00 x 10-4; Ka2 = 1.00 x 10-8; Vol=0.01000 L; FH2A=0.1000 M) and the titrant is a strong monoprotic base..
The second-order reaction 2 Mn(CO)5 Mn2(CO)10, has a rate constant equal to 3.0 x 10^9 M-1 s-1 at 25C. If the initial concentration of Mn(CO)5 is 2.0 x 10-5 M, how long will it take for 90.% of the reactant to disappear?
If you dilute 33.4 mL of a 3.5 M solution to make 244.0 mL of solution, what is the molarity of the dilute solution.
Ammonia and hydrogen chloride gases react to form solid ammonium chloride. A 10.0 L reaction flask contains ammonia at 0.450 atm and 22°C, and 164 mL of hydrogen chloride gas at 7.50 atm and 271 K is introduced
construct an energy level diagram (molecular orbital) for the molecule SO. We are then asked to comment on the ionic species of SO - bond order, bond distance etc. So far so good.
22.5ml of .383 molar H2SO4 is required to completely neutralize 20ml of KOH solution. What is the molarity of the KOH solution?
Calculate the volume of a solution NaOH c=0.2 mol/l necessary to neutralize v=200 ml of solution HCl c=0.1 mol/l.
whats the concentration of the acetic acid solution? If 10.91 mL of an acetic acid solution required 9.78 mL of 1.0439 M NaOH
Fundamentals of chemistry - The conditions under which gases behave most ideally and Under the Bronsted?Lowry definition a base
A solution is prepared by adding 60.0 mL of 0.060 M HBr to 180.0 mL of 0.70 M HI. Calculate the concentrations of all species in this solution. HBr and HI are both considered strong acids
What is the pH of this buffer after 0.45 mL of 10.0 M hydrochloric acid are added to it? The Ka for HF is 6.8 x 10-4.
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