Calculate the pH of 1.00 L of a solution that is 0.120M in HNO₂ and 0.150M in NaNO₂ before and after you add 2.0mL of 15.0M HCL. [K_a(HNO₂) = 4.0 x 10^-4]

Prove that Inter energy is Independent of the path

a buffer solution is prepared by mixing 100cm3 aqueous NH3 0.1mol dm-3 with 100cm3 NH4Cl mol dm-3 . Given that KB for NH3 =1.74x10^-5
...
1) calculate pH of the buffer solution.
...
2)calculate the solution after addition 50cm3 HCl of 0.1 mol dm-3.

what volume of 0.305 M AgNO3 is required to react exactly with 155.0 ml of 0.274 Monday Na2SO4 solution?

a 0.1965g sample containing copper is analysed iodometrically. copper(ii) is reduced to copper(i) by iodide:

2Cu2+ + 4I- --> 2Cul + I2

calculate the percentage of copper in the sample if 25.0mL of 0.1005M Na2S2O3 is required for the titration of the liberated iodine.

After Carrying out the Aspirin synthesis experiment, Suggest an experiment or technique based on what you have learned in the last few weeks to confirm the preparation of Aspirin. (Give full details) Hint: You are provided with pure sample of Aspirin  

Draw the structure of a compound with the formula C9H20 that has two non-adjacent chirality centers, both S.

As a food chemist for a major potato chip company, you are responsible for determining the salt content of new potato chip products for the packaging label. The potato chips are seasoned with table salt, NaCl. You weigh out a handful of the chips, boil them in water to extract the salt, and then filter the boiled chips to remove the soggy chip pieces. You then analyze the chip filtrate for Cl− concentration using the Mohr method.

First you prepare a solution of silver nitrate, AgNO3, and titrate it against 0.500 g of KCl using the Mohr method. You find that it takes 64.9 mL of AgNO3 titrant to reach the equivalence point of the reaction.

You then use the same silver nitrate solution to analyze the chip filtrate in a Mohr reaction, finding that the solution yields a rusty brown precipitate when 48.2 mL of titrant is added.

Part A

If the sample of chips used to make the filtrate weighed 83.0 g , how much NaCl is present in one serving (155 g ) of chips?

Express your answer to three significant figures and include the appropriate units.

Will a precipitate form if 100.0 mL of 2.5 × 10−3M Cd(NO3)2 and 75.0 mL of 0.0500 M NaOH are mixed at 25°C? Calculate the concentration of cadmium ion in solution at equilibrium after the two solutions are mixed. (Ksp is 7.2 × 10−15 for Cd(OH)2 at 25°C)

Most of our discussion of transition metals has focused around them becoming positively charged ions. However, many of the transition metals will also become negatively charged ions. Using what you have learned from quantum mechanics and about electron configurations, predict which transition metals are most likely to form anions with a charge of -1 and explain the prediction.

5) The following example illustrates an ammonia synthesis process in which an inert gas (I) is present, necessitating a purge stream. The fresh feed to the process contains nitrogen and hydrogen, as well as an inert gas (I). The feed is combined with a recycle stream containing the same three species, and the combined stream is fed to a reactor. The reactor effluent flows to a condenser. A liquid stream containing all of the ammonia formed in the reactor and a gas stream containing all the inerts and the unreacted nitrogen and hydrogen leave the condenser. The gas stream is split into two fractions with the same composition: one is removed from the process as a purge stream, and the other is the recycle stream, which is subsequently combined with the fresh feed. In every stream containing nitrogen and hydrogen, the two species are in stoichiometric proportion. Let yI0 be the mole fraction of inerts in the fresh feed, f the single-pass conversion of nitrogen in the reactor, and p the fraction of the gas leaving the condenser that is purged (mol purged/mol total). Draw and fully label a process flowchart, and using stoichiometric ratios, physical constraints and simple material balances in your head, try to introduce the fewest possible variables. In other words express as many quantities as possible in terms of yI0, f and p. Given yI0 = 0.01, f = 0.20, and p = 0.10, chose a basis anywhere in the problem and solve for the total moles fed to the reactor (nr), moles of ammonia produced (np), and overall nitrogen conversion (fov).

Calculate the solubility (a) in mol/L and (b) in g/L of AgCl in 2.0 M NH3(aq). What is the concentration of Ag+ in this solution? (Ksp = 1.6 x 10-10; Kf = 1.7 x 107 for Ag(NH3)2+

Calculate the pH at the equivalence point in titrating 0.011 M solutions of each of the following with 0.054 M NaOH.

(a) hydrobromic acid (HBr)

(b) phenol (HC6H5O), Ka = 1.3e-10

(c) hypoiodous acid (HIO), Ka = 2.3e-11

A solution that may contain Cu²⁺, Bi³⁺, Sn⁴⁺, or Sb³⁺ ions is treated with thioacetamide in an acid medium. The black precipitate that forms is partly soluble in strongly alkaline solution. The precipitate that remains is soluble in 6 M HNO₃ and gives only a blue solution on treatment with excess NH₃. THe alkaline solution, when acidified, produces, an orange precipitate. On the basis of this information, which ions are present, which are absent, and which are still in doubt?