1. Determine the amount of solute in the following samples:
500 ml of 0.2 M KI (potassium iodide)
220 ml of 0.03 M H2SO4 (sulfuric acid)
2.5 l of 0.1 M MgNO3 (magnesium nitrate)
1 ml of 5 M HCl (hydrochloric acid)
This problem requires that you know what molarity (M) is. M (molarity) = # of moles of solutes / Liter of solution. You are given the volume. You should be able to obtain moles of solutes. Your answers can be in moles or grams (either one will be acceptable).
2. How many ml of 0.1 M HCl would be required to titrate 35 ml of 1 M NaOH to the end point?
This is an acid/base reaction.
1) First, write out the balanced chemical reaction for HCl + NaOH.
2) Second, figure out the number of moles of NaOH in 35 ml of 1 M NaOH.
3) How many moles of HCl is required for completely reacting with the moles of NaOH in Part 2).
3. What is the pH of a 0.03 M solution of the strong base NaOH?
1) This question requires that you know pH = - log [H3O+], or simply as pH = - log [H+] (to make it easier).
2)So, you have to know how to use your scientific calculator to do log function (check Youtube).
3) This question also requires that you know: pOH = - log [OH-].
4) This question also requires that you know: [H3O+][OH-] = 1.0 x 10-14 or pH + pOH = 14
5) First step, determine the concentration of OH- in 0.03M NaOH when it dissociates or breaks up into Na+ and OH-.
6) This will give you [OH-]. You can plug this into pOH = - log [OH-] to get pOH.
7) Once you get pOH, then use (pH + pOH = 14) to get pH.
4. Balance the chemical reactions shown below and then write equilibrium expressions for each. All reactants and all products are in the gas phase.
CO + F2 ------> COF2
CH4 + O2 ------> CO2 + H2O
N2O4 -----> Br2 + NO
BrNO -----> Br2 + NO
1)This problem requires that you know how to balance chemical equations.
2)After you balance the equation, you need to know the equilibrium expression
5. Determine the oxidation states of each element comprising the following ionic compounds:
KClO4
NaMnO4
Sr(NO3)2
NaHCO3
CH4
