HClO is a weak acid (Ka = 4.0 × 10–8) and so the salt NaClO acts as a weak base. What is the pH of a solution that is 0.017 M in NaClO at 25 °C
In: Chemistry
1.For the reaction,
PCl5(g) <-----> PCl3(g) + Cl2(g) Kp = 24.6 at 500 K
calculate the equilibrium partial pressures of the reactants and
products if the initial pressures are PPCl5 =
0.610 atm, PPCl3 = 0.400 atm and
PCl2 = 0.000 atm.
PPCl5 = PPCl3 = PCl2 =
2.
H2O(g) + Cl2O(g) <-----> 2HClO(g) Kc = 0.14 at 298.15 K
calculate the equilibrium concentrations of the reactants and
products if the initial concentrations are [H2O(g)] =
0.00482 mol L-1, [Cl2O(g)] = 0.00482 mol
L-1 and [HClO(g)] = 0.000 mol L-1.
[H2O(g)] = [ClO2(g)] = [HClO(g)] =
3.A flask that initially contained pure NO2 was
heated to 1000 K, a temperature at which the value of Kp
for the decomposition of NO2 is 128.8.
2NO2(g) <-----> 2NO(g) + O2(g)
Given that the partial pressure of O2 at equilibrium
equals 0.168 atm calculate the partial pressures of NO2
and NO at equilibrium.
PNO = PNO2 =
4.The equilibrium constant Kp for the
reaction,
2 SO3(g) <-------> 2 SO2(g) + O2(g)
is 8.440 at 789 °C. If a vessel at this temperature initially
contains pure SO3 and if the partial pressure of
SO3 at equilibrium is 0.050 atm, what is the partial
pressure of O2 in the flask at equilibrium?
What was the initial pressure of SO3 in the flask?
In: Chemistry
Calculate the percent dissociation of HF (Ka= 3.5x10^-4) in
(a) 0.050 M HF
(b) 0.50 M HF
In: Chemistry
Write:
a) balanced equation
b) total ionic equation
c) net ionic equation
d) type of reaction
e)limiting reactant
1) Cu(s) + HNO3(aq) -> Cu(NO3)2 (aq)+ NO2(g) +H2O(l)
2) Cu(NO3)2(aq) + NaOH(aq) -> Cu(OH)2(s) + NaNO3
3) Cu(OH)2(s) -> CuO(s) +H2O
4) CuO(s) + H2SO4(aq) ->CuSO4(aq) +H2O(l)
5)CuSO4(aq) + Zn(s) -> Cu(s) +ZnSO4 (aq)
In: Chemistry
Calculate enthalpy for the following reaction Ca(s) + 1/2O2 + CO2 = CaCo3 Given the following reactions: Ca(s) + 1/2 O2 = CaO (s) H= -635.1 kj CaCo3 = CaO (s) + CO2 H= 178.3 kj
In: Chemistry
Consider a solution formed by mixing
50.0 mL of 0.100 M H2SO4,
30.0 mL of 0.1000 M HOCl,
25.0 mL of 0.200 M NaOH,
25.0 mL 0.100 M Ba(OH)2, and
10.0 mL of 0.150 M KOH.
Calculte the pH of this solution.
Ka (HOCl) = 3.5 x 10-8
What is the pH?
In: Chemistry
Chromatography explained in details highlighting important things to know for test.
In: Chemistry
Exothermic Vs. Endothermic Reaction
Reaction progress diagrams for single-step endothermic and exothermic reactions.
a. Devise a general statement about the relationship between Ea and the rate of a reaction.
b. Describe the effect of temperature on the energy of collisions, and explain how this effect changes the rate of a reaction.
c. State three things that resulted in an increase in the rate of the reaction. For each of the three things, explain at a molecular level what happens to cause the rate of the reaction to increase.
In: Chemistry
A 12.9 mL solution of 0.100 mol L-1 HOCl is titrated using 0.150 mol L-1 NaOH.
What is the pH of the solution after 5.18 mL of the NaOH solution is added? Express your answer to 2 decimal places.
You have 5 attempts at this question.
Remember you can find KA and/or KB values in your textbook in chapter 15.
In: Chemistry
In: Chemistry
A saturated solution of barium fluoride, BaF2, was prepared by dissolving solid BaF2 in water. The concentration of Ba2+ ion in the solution was found to be 7.52
In: Chemistry
Compare and contrast the different types of chemical bonds and define the terms chemical bond, covalent bond (including polar and nonpolar), ionic bond, and hydrogen bond.
In: Chemistry
Balance each reaction, determine if they are ion-exchange, redox, or acid-base, and determine the direction of the reaction and if they are reverisble or irreversible and explain why.
NH4 NO(s) – N(g) + H2(g)
N2 (g) + O2 (g) – NO (g)
N2 (g) + H2 (g) – NH3 (g)
H2O (g) - O2 (g) + H2 (g)
CaCO3 (s) – CaO (s) + CO2 (g)
Cl2 (g) + H2O (l) – HCl (aq) + HClO (aq)
NH4 (s) – NH3 (g) + HCl (g)
Fe (s) + H2SO4 (aq) – FeSO4 (aq) + H2 (g)
CO2 (g) + H2O (l) – H2CO3 (aq)
Mg (s) + H2O (l) – Mg(OH)2 (aq) + H2 (g)
CH3-COOH (aq) + H2O (l) - CH3-COO- (aq) + H3O+(aq)
In: Chemistry
Write the formula of the coordination compound pentacarbonyliron(0)
Write a systematic name for Li2[CoF6].
Write a systematic name for [RuCl2(bipy)2].
Write a systematic name for [Co(NH3)3Cl3].
In: Chemistry
9.) As mentioned below, you are required to design your own procedure for determining the heat of dissolution of your chosen salt with a coffee cup calorimeter. Answer the following questions and consider them in designing this procedure:
a.) When you find your initial temperature Ti, should you take one measurement from the thermometer as soon as you place it in the water in the calorimeter? Why or why not? If not, what should you do instead?
b.) Do you expect the temperature of the water in the calorimeter to rise, fall, or stay the same after you add your salt? If the temperature will change, will it continue to change indefinitely or not?
c.) How will you know your dissolved salt solution has reached it's maximum or minimum temperature, i.e. what will you observe in your data to indicate this has happened?
d.) Should you repeat your experiment? Why or why not? If so, what could you change from trial to trial? Give two possible suggestions, and determine which one you should change (as well as which one you should not!) in any subsequent trials you decide to perform.
*Information previously calculated is below*
1. Calculate the amount of heat (q) produced by the combustion of 4.05 g CH4 (ΔHcomb = -890.4 kJ).
225.38 kj
2. Consider that the 4.05 g methane is burned and all of the heat from this combustion is absorbed by 1.0 kg of 20 °C water (use 4.18 g-1 ºC-1 for the specific heat of the water). What would be the final temperature of the water?
73.8°C
In: Chemistry