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Consider the reaction of 25.0 mL of 0.20 M AgNO3(aq) with 25.0 mL of 0.20 M NaBr(aq) to form AgBr(s) at 25°C: Ag+(aq) + Br-(aq) ? AgBr(s). What is ΔG for this reaction? The Ksp of AgBr is 5.0 x 10^-13 at 25°C.
0.75 g of hydrogen chloride (HCl) is dissolved in water to make 7.0 L of solution. What is the pH of the resulting hydrochloric acid solution.
If a gas held at constant pressure had an initial volume of 5.00 L and the temperature changed from 35°C to 578 K what would be the final volume of this gas?
what molecule would give the following mass spec data. this molecule shows three significant fragment ions. Alpha-fragmentation forms the m/z =59 base peak
Xenon can be the central atom of a molecule by expanding beyond an octet of electrons. Draw Lewis structure for the following xenon compound.
Given a buret filled with 0.12 M acetic acid and a second buret filled with 0.15 M sodium acetate, how many milliliters of each solution should be mixed together to produce 21.0 mL of a solution with a pH of 4.70
How many molecules of carbon dioxide are produced when 121 molecules of acetylene (HCCH) to react in excess oxygen produce carbon dioxide and water?
When a 19.7 mL sample of a 0.323 M aqueous hydrofluoric acid solution is titrated with a 0.399 M aqueous potassium hydroxide solution, what is the pH at the midpoint in the titration
Compute the [H+] and pH of a 0.0040 M hydrofluoric acid solution. Remind that the Ka of hydrofluoric acid is 6.8 × 10-4. Utilize the method of successive approximations in your calculations.
Helium is the lightest noble gas component of air and xenon is the heaviest. Use R=8.314J(mol x K) and M in kg/ml. Find the rms speed of helium in 0 degree C and in 30 degree C
sodium hydroxide to make sodium phosphate and water. How many L of the H3PO4 solution will react with 0.281 L of the NaOH solution? Give your answer to 3 decimal places.
If 31.0 mL of 34.0% hydrochloric acid solution (density = 1.17g/mL) is diluted with water to a volume of 1.50 L, what is the concentration of the diluted solution
In the titration of a weak base (0.100 M piperazine, 40 mL) with a strong acid (0.100 M HCl). Calculate the pH values between 0 mL Va and 100 mL in 10 mL steps. The two Ka values of piperazine are 4.65 x 10^-6 and 1.86 x 10^-10
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