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2. Rust stains can be removed by washing a surface with a dilute solution of oxalic...
one practical application of oxalic acid (H2C2O4) is as a rust remover. Rust is primarily composed...
one practical application of oxalic acid (H2C2O4) is as a rust remover. Rust is primarily composed of Fe2O3, which reacts with oxalic acid according to the unbalanced equation shown below. Fe2O3 (s) + H2C2O3 (aq) --> Fe(C22O4)3-3 (aq) + H2O (l) + H+ (aq) Calculate the number of milligrams of Fe2O3 that can be removed using 500.0 mL of 0.1068 M H2C2O4.
One of the uses of oxalic acid, (H2C2O4) is rust removal. It reacts with rust, (Fe2O3)...
One of the uses of oxalic acid, (H2C2O4) is rust removal. It reacts with rust, (Fe2O3) according to the equation: 2Fe2O3(s) + 6H2C2O4(aq) = 2Fe2(C2O4)3^-3(aq) + 3H2O(l) + 6H+(aq) Calculate the number of grams of rust that can be removed by 5x10^2mL of a 0.100 mol L-1 solution of oxalic acid.
6. Oxalic acid H2C2O4 is a diprotic acid and can be used, in dilute form, as...
6. Oxalic acid H2C2O4 is a diprotic acid and can be used, in
dilute form, as wood bleach. pKa1 = 1.237 and pKa2=4.187
A. How many milliliters of 0.0500 M NaOH would be required to
completely neutralize 10.0 mL of 0.100 M H2C2O4? (5 pts)
B. Estimate the pH at the first equivalence point of the
titration. (6 pts)
C. What is the pH at the second equivalence point of the
titration. (8 pts)
Please help with work shown, especially...
04 (a) Calcium ions can be determined by precipitation of the oxalate according to the equation:...
04 (a) Calcium ions can be determined by precipitation of the oxalate according to the equation: Ca2+ (aq) + C2O42- (aq) = CaC204 (s) The solid may then be filtered off, washed and oxalic acid is regenerated by the addition of excess sulfuric acid. The amount of oxalic acid is then quantified by titration using potassium permanganate according to the equation: H2C204 + MnO4 + H+ = CO2 + Mn2+ + H20 (unbalanced) In an experiment to find the concentration...
b. Determine what mass of rust can be removed by 540 g of oxalic acid? ....
b. Determine what mass of rust can be removed by 540 g of oxalic acid? . Cyanogen, C2N2 is a colorless, poisonous gas that can be prepared by the following: +2 CuCN (a) CN2(+2 K,SO4 (ag) 2 CuSO4 () +4 KCN (a) o a. Determine how many moles of KCN are required to react with 3.7 moles of CuSO4 b. Determine how many moles of cyanogen are produced from 1.75 moles of CuSO4 c. Determine how many moles of K2SO4...
HW 14 <Question 24 (of 29) 0.68 points 10 attempts left Check my work Enter your answer in the provided box. In a dilute nitric acid solution, Fe' reacts with thiocyanate ion (SCN) to form...
HW 14 <Question 24 (of 29) 0.68 points 10 attempts left Check my work Enter your answer in the provided box. In a dilute nitric acid solution, Fe' reacts with thiocyanate ion (SCN) to form a dark red complex: [Fe(H2O)6]3t + SCN-→ H2O + [Fe(H2O)sNCS] 2+ The equilibrium concentration of [Fe(H,oNCSmay be determined by how dark the colored solution is (measured by a spectrometer). In one such experiment, 1.0 mL of 0.20 M Fe(NO)s was mixed with L.0 mL of...
1. What is the pH of a solution made by mixing 100.mL each of two solutions...
1. What is the pH of a solution made by mixing 100.mL each of two solutions of HCl(aq), one with pH = 2.00 and one with pH = 3.00? 2. What volume of 0.150M NaOH is required to reach the endpoint in the titration of 25.00mL of 0.0850M H2C2O4? Note that oxalic acid is diprotic. 3. Indicate whether the each of the following chemical reactions are A) A Lewis acid/base reaction, B) An acid/base reaction, but not a Lewis acid/base...
Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV)...
Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide. 4 HCl(aq) + MnO,(s) —MnCl(aq) + 2 H2O(l) + Cl2(g) A sample of 42.1 g Mno, is added to a solution containing 42.1 g HCI. What is the limiting reactant? MnO2 OHCI What is the theoretical yield of CI,? theoretical yield: CI, If the yield of the reaction is 77.5%, what is the actual yield of chlorine? actual yield: g CI Dimethyl oxalate,...
Additional Problem 6.098 Your answer is partially correct. Try again. A dilute solution of hydrochloric acid...
Additional Problem 6.098 Your answer is partially correct. Try again. A dilute solution of hydrochloric acid with a mass of 614.08 g and containing 0.30664 mol of HCl was exactly neutralized in a calorimeter by the sodium hydroxide in 618.91 g of a comparably dilute solution. The temperature increased from 16.663 to 19.946 °C. The specific heat of the HCl solution was 4.031 Jug-1.°C-1; that of the NaOH solution was 4.046 Jug-1.00-1. The heat capacity of the calorimeter was 77.99...
Acidic solution In acidic solution, the iodate ion can be used to react with a number...
Acidic solution In acidic solution, the iodate ion can be used
to react with a number of metal ions. One such reaction is
IO3−(aq)+Sn2+(aq)→I−(aq)+Sn4+(aq) Since this reaction takes place
in acidic solution, H2O(l) and H+(aq) will be involved in the
reaction. Places for these species are indicated by the blanks in
the following restatement of the equation: IO3−(aq)+Sn2+(aq)+
−−−→I−(aq)+Sn4+(aq)+ −−−
Part A-
What are the coefficients of the reactants and products in the
balanced equation above? Remember to include H2O(l)...
6. Oxalic acid H2C2O4 is a diprotic acid and can be used, in
dilute form, as wood bleach. pKa1 = 1.237 and pKa2=4.187
A. How many milliliters of 0.0500 M NaOH would be required to
completely neutralize 10.0 mL of 0.100 M H2C2O4? (5 pts)
B. Estimate the pH at the first equivalence point of the
titration. (6 pts)
C. What is the pH at the second equivalence point of the
titration. (8 pts)
Please help with work shown, especially...
04 (a) Calcium ions can be determined by precipitation of the oxalate according to the equation: Ca2+ (aq) + C2O42- (aq) = CaC204 (s) The solid may then be filtered off, washed and oxalic acid is regenerated by the addition of excess sulfuric acid. The amount of oxalic acid is then quantified by titration using potassium permanganate according to the equation: H2C204 + MnO4 + H+ = CO2 + Mn2+ + H20 (unbalanced) In an experiment to find the concentration...
b. Determine what mass of rust can be removed by 540 g of oxalic acid? . Cyanogen, C2N2 is a colorless, poisonous gas that can be prepared by the following: +2 CuCN (a) CN2(+2 K,SO4 (ag) 2 CuSO4 () +4 KCN (a) o a. Determine how many moles of KCN are required to react with 3.7 moles of CuSO4 b. Determine how many moles of cyanogen are produced from 1.75 moles of CuSO4 c. Determine how many moles of K2SO4...
HW 14 <Question 24 (of 29) 0.68 points 10 attempts left Check my work Enter your answer in the provided box. In a dilute nitric acid solution, Fe' reacts with thiocyanate ion (SCN) to form a dark red complex: [Fe(H2O)6]3t + SCN-→ H2O + [Fe(H2O)sNCS] 2+ The equilibrium concentration of [Fe(H,oNCSmay be determined by how dark the colored solution is (measured by a spectrometer). In one such experiment, 1.0 mL of 0.20 M Fe(NO)s was mixed with L.0 mL of...
Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide. 4 HCl(aq) + MnO,(s) —MnCl(aq) + 2 H2O(l) + Cl2(g) A sample of 42.1 g Mno, is added to a solution containing 42.1 g HCI. What is the limiting reactant? MnO2 OHCI What is the theoretical yield of CI,? theoretical yield: CI, If the yield of the reaction is 77.5%, what is the actual yield of chlorine? actual yield: g CI Dimethyl oxalate,...
Additional Problem 6.098 Your answer is partially correct. Try again. A dilute solution of hydrochloric acid with a mass of 614.08 g and containing 0.30664 mol of HCl was exactly neutralized in a calorimeter by the sodium hydroxide in 618.91 g of a comparably dilute solution. The temperature increased from 16.663 to 19.946 °C. The specific heat of the HCl solution was 4.031 Jug-1.°C-1; that of the NaOH solution was 4.046 Jug-1.00-1. The heat capacity of the calorimeter was 77.99...
Acidic solution In acidic solution, the iodate ion can be used
to react with a number of metal ions. One such reaction is
IO3−(aq)+Sn2+(aq)→I−(aq)+Sn4+(aq) Since this reaction takes place
in acidic solution, H2O(l) and H+(aq) will be involved in the
reaction. Places for these species are indicated by the blanks in
the following restatement of the equation: IO3−(aq)+Sn2+(aq)+
−−−→I−(aq)+Sn4+(aq)+ −−−
Part A-
What are the coefficients of the reactants and products in the
balanced equation above? Remember to include H2O(l)...
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