25.0 mL of 2.8 M NH3(aq) was added to 20.0 mL of 1.5 M HCl(aq) and the mixture was stirred, then tested with a pH meter. Complete the following table based on the reaction. NH3 HCI NH4CI Beginning/mol choose yo v choose ycv choose your an Reaction/mol choose yo choose y

What two quantities are equal at the endpoint of a titration of an antacid? O number of molecules of acid = number of molecules of base %D O grams of acid = grams of base %3D O moles of acid = moles of base O volume of acid = volume of base

You dissolve a 0.250 M solution of sodium acetate. You then titrate 25.0 mL of that solution with 0.200 M HNO3. Determine the pH that will be measured (a) initially, (b) after 20.0 mL, (c) after 31.25 mL, and (d) after 35.00 mL of HNO3 has been added. The Ka for acetic acid is 1.8 x 10^-5

What will happen if the pH of the following equilibrium system is increased? H*(aq) + 2CrO4²a yellow The solution will turn yellow. b. The solution will turn a darker orange. There will be no effect on the equilibrium system. 2- aq) O Cr20,² (aq) + OH (аq) orange а. с. d. The concentration of OH will decrease. (aq) All hydroxide ion will be used up. е.

Paylben

A buffer solution contains 0.387 M NaH,PO4 and 0.212 M K2HPO4. Determine the pH change when 0.061 mol HCIO, is added to 1.00 L of the buffer. pH change =| A buffer solution contains 0.229 M CGH;NH3CI and 0.381 M C,H3NH2 (aniline). Determine the pH change when 0.077 mol HCl is added to 1.00 L of the buffer. pH after addition – pH before addition = pH change =| A buffer solution is 0.301 M in HCN and 0.274 M in KCN . If K, for HCN is 4.0×10-10 , what is the pH of this buffer solution?

65.0 mL of 0.575 M HNO, is titrated by 0.450 M KOH. Calculate the pH of the acid solution before any titrant is added. pH = 0.240 Calculate the pH after 50.29 mL of 0.450 M KOH is added to 65.0 mL of 0.575 M HNO pH = 0.882 3 Calculate the pH after 83.06 mL of 0.450 M KOH is added to 65.0 mL of 0.575 M HNO3. pH = 9.10 Calculate the pH after 154 mL of 0.450 M KOH is added to 65.0 mL of 0.575 M HNO3. pH = 13.18

A solution may contain any or all of the following cations: Ag+, Pb2+, Ba2+, Ni2+ in an UNKNOWN mixture. HCl is added to the solution and a precipitate forms. That precipitate is removed and NH3 (aq) is added to the supernatant until the solution is basic, no solid forms. After making the supernatant basic, K2CrO4 is then added and a precipitate forms. What cations (Ag+, Pb2+, Ba2+, Ni2+)are present in this unknown sample (This is chemistry and not a writing question)

21- The mass-action effect is a shift in the position of an equilibrium caused by adding one of the reactants or products to a system. O True O False 20- Buffer solution is a mixture of a weak acid and it's salt. or weak base and it's salt. the pH of buffer resists change upon adding small amount of strong acid or base or when it dilute. O True O False I 22- Equilibrium-constant are algebraic equations that describe the concentration relationships among reactants and products at equilibrium O True O False ترك السؤال ترك السؤال ارسال الاجابة ارسال الاجابة

A sample of acetic acid is titrated with a standardized NAOH solution. Before the end-point of the titration, which of the following must be true? HC,H3O, (aq) + NAOH (aq) → NaC,H3O2 (aq) + H2O (1) Note: [X] = molar concenctration of X %3D O [H+] > [OH-] [-HO] > [+H] O %3D [-HO] = [+H] O