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Calculate the concentration of all the species, ions, and molecules, and the pH of the following solutions. All solutions have a total volume of 1.00 liter and contain: (Please show work so I can solve other similar problems) A) 0.10 mole HClO (Ka=3.0x10^-8) B) 0.20 mole NH3 (ammonia Kb=1.8x10^-5) C) 0.10 mole NaClO (HClO <---> H+ + ClO-; Ka=3.0x10^-8) D) 0.10 mole KNO2 (HNO2 <---> H+ + NO2-; Ka=5.1x10^-4)
Describe the steps to be taken in the laboratory if a large bottle of acetone (noncorrosive, nontoxic, highly volatile, water-soluble, flammable solvent) is broken and spilled.
The molar heat of combustion of methanol (molar mass = 32.0g/mol) is -757kJ/mol. If 2.00 g of methanol is placed in a bomb calorimeter with a heat capacity of 6.50 kJ/degree C what is the temperature rise when the sample is combusted?
The decomposition of ozone in the upper atmosphere is facilitated by {\rm NO}. The overall reaction and the rate law are O3(g) + O(g) = 2 O2(g) Rate = k [ O3}][ NO]
the partial pressure of oxygen in the atomsphere is 0.20 atm, what is the solubility of dissovled oxygen in blood? recall that the soulibilty of oxygen constant
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 0.087 M in NaClO?
What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous formic acid requires 29.80 mL of 0. 3567 M NaOH? Ka =1.8 × 10-4 for formic acid.
If 10.00 mL of 0.250 M NaOH solution is added to 100.00 mL of the above original buffer solution (described in part 1 of this problem), what is the new pH of the solution?
The atmospheric oxidation of nitrogen monoxide was studied at 183C with initial partial pressure of 1.000 atm of NO and 1.000 atm of O2. At equilibrium, Po2= .50-6 atm. Calculate Kp. 2 NO(g) +02 ->
A gas cylinder at a pressure of 5.80 atm contains both helium and oxygen. The helium is at a pressure of 2.35 atm. What is partial pressure of oxygen?
what is the molarity of a saturated solution of AgOH with a Ksp = 2.0 x 10^ -8
What mass of NaOH can this buffer neutralize before the pH rises above 4.00?
A laboratory method of preparing oxygen gas involves decomposition of solid potassium chlorate. The products of the reaction are solid potassium chloride and oxygen gas.
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