14) you are titrating 10.0mL of a solution of 0.25M acetic acid (Ka=1.8 x 10 ^-5). you are using a solution of 0.10M KOH to complete the titration curve. create the graph that would result by adding 1.0mL of the base to the acid and determining the pH and repeating until you have passed the equivalence point. Start the graph with 0 mL of the base solution added.  

2. Which of the following gases could have the same pressure and temperature? All of the containers are rigid and have the same volume.

A.Ne and N2

B.O3 and H2O

C.N2 and O3

D. Ne, N2, and H2O

Calculate the pH of a buffer that is 0.10 M in KH2PO4 and 0.050 M in Na2HPO4. What is the pH after adding 5.0 mL of 0.20 M HCl to 0.10 L of this buffer. The Ka value for H2PO4– is 6.32 × 10–8 or a pKa of 7.199

What does the titration curve for 5ml pH 5.6 acetate buffer being titrated with 1.5M NaOH look like?

What is the buffer capacity?

What volume is needed to change pH from initial pH to neutralization etc.

If the gas-solid equilibrium amounts to a monolayer capacity of 150cc(STP)/g of N2 (16.2e -20 m^2/ molecule), the surface area of 1g of the solid adsorbent exceeds 850 m^2. True or False?

10) You want to create a buffer using phosphoric acid and Sodium Dihydrogen Phosphate. what is the best pH at which to make the buffer? using that pH and a concentration of 1M. Determine the molar concentrations of each component (acid and base) needed to make the buffer. If you need 100mL of the buffer, how many mL of 2.5 M phosphoric acid will you need? How many grams of the Sodium Dihydrogen Phosphate do you need?

11) using the buffer you created in problem 10 calculate the change in pH if you add 1 mL of 0.50M HCl to the buffer.

12) using the buffer you created in problem 10. calculate the change in pH if you add 2 mL of 0.50 NaOH to the buffer.

1. Often you may have seen results of an experiment, such as blood analysis, reported as “counts”. (a) What type of results may be represented by counts? Hint: there’s more than one type.

Assuming complete dissociation, what is the pH of a 4.21 mg/L Ba(OH)2 solution?

pH=

Calculate the solubility of LaF3 (Ksp = 2 x 10-19) in grams per liter in: a) pure water b) 0.010 M KF solution

if a titration using these solutions started with 25.00 mL of potassium chromate solution (0.5056 M), what volume of 0.2456 M lead (II) nitrate solution would be required to reach the end point? what MASS of the products would be created in that reaction?

Calculate % yield of triphenylmethanol (crude and pure)

Remember it is a two step calculations, so you should obtain the following to aid in the calculations: the mass of first reagent, mass of second reagent (including HCl – Vol & Density), and moles of both reagents (for each procedure). Then set up a Balanced Stoichiometric Equation, determine the molar ratio, determine limiting reagent and compute the theoretical yield.

These are the values:
Bromobenzene + Magnesium --> Phenylmagnesium Bromide

Phenylmagnesium Bromide + Benzophenone ---> Triphenylmethanol + Magnesium Bromide Hydroxide

0.1538g of Mg 0.9mL Bromo/Ether solution 1.0910 benzophenone + 2mL ether —-> 0.349g

   6mL of 6M HCl 2mL diethyl ether 0.301g triphenylmethanol (recrystalized and weighed 0.201 g triphenylmethanol)

What is the difference between an electrochemical cell and a voltaic cell? Is there any? If they are different how do each of their electrons flow?