What is the initial pH, at half way and after 12.5 mL of NaOH 0.3235 M is used to titrate 65.00 mL of 0.1237 M HAc?    Ka=1.75 x 10^-5

For calcite dissolution experiment, when you increase ionic strength from 0 (infinite diluted) to 0.1 m, how much does the solubility increase？

At 650 K, the reaction MgCO3(s)?MgO(s)+CO2(g) has Kp=0.026. A 12.5L container at 650 K has 1.0 g of MgO(s) and CO2 at P = 0.0260 atm. The container is then compressed to a volume of 0.500L . Find the Mass of MgCO₃ that is formed

A titration is a procedure for determining the concentration of a solution by allowing it to react with another solution of known concentration (called a standard solution). Acid-base reactions and oxidation-reduction reactions are used in titrations. For example, to find the concentration of an HCl solution (an acid), a standard solution of NaOH (a base) is added to a measured volume of HCl from a calibrated tube called a buret. An indicator is also present and it will change color when all the acid has reacted. Using the concentration of the standard solution and the volume dispensed, we can calculate molarity of the HCl solution.

Part A

A volume of 70.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 17.7 mL of 1.50 M H2SO4 was needed? The equation is

2KOH(aq)+H2SO4(aq)→K2SO4(aq)+2H2O(l)

Express your answer with the appropriate units.

Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, H2O2, can be titrated against a solution of potassium permanganate, KMnO4. The following equation represents the reaction:

2KMnO4(aq)+H2O2(aq)+3H2SO4(aq)→3O2(g)+2MnSO4(aq)+K2SO4(aq)+4H2O(l)

A certain amount of hydrogen peroxide was dissolved in 100. mL of water and then titrated with 1.68 M KMnO4. What mass of H2O2 was dissolved if the titration required 18.3 mL of the KMnO4 solution?

Express your answer with the appropriate units.

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.