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Calculate the percentage...
Calculate the molarities and normalities of the following solutions. The reactions are those given in problem...
Calculate the molarities and normalities of the following solutions. The reactions are those given in problem 1. 4.50 g of Hg(NO3)2 in 150.0 mL of solution 15.0 g of Ba(OH)2 in 1.15 L of solution 12.0 g of KCN in 200 mL of solution A solution of sodium thiosulfate, Na2S2O3 is standardized using pure potassium dichromate, K2Cr2O7, as the primary standard. A sample of K2Cr2O7 weighing 0.2263 g was dissolved, acidified, and excess KI added to liberate I2. The I2...
Given the following data: C) IT final init (°C) H2O 50.00 ml 21.40 22.28 Na2S203 3.25...
Given the following data: C) IT final init (°C) H2O 50.00 ml 21.40 22.28 Na2S203 3.25 g Calculate AHº for the reaction: Na2S2O3(s) - Na2S2O3(aq) You may assume all solutions to have the same density and specific heat as water (1.00 g/mL and 4.184 J/g°C) kJ/mol
calculate tbe hardness of the water given expeirmental data 25 mL of water was used Part 2: The Hardness of Water...
calculate tbe hardness of the water given expeirmental data
25
mL of water was used
Part 2: The Hardness of Water Samples Experimental Data Concentration of EDTA O.OLOS N #2-Tap #5- Mineral Sample number #1- Tap # 4-Mineral #3-Mineral 2245 23.10 35.32 33 2 2 34, ss Initial burette reading 19.us 00 43.10 Final burette reading 23.10 22ur Reaction M2 (aq) +EDTA (aq) [M(EDTA) ] (aq) where M2 Ca2 and Mg Calculated Values #1- Tap #5-Mineral #2-Tap #4-Mineral #3-Mineral Volume...
A 0.450 g sample of impure CaCO, (s) is dissolved in 50.0 mL of 0.150 M...
A 0.450 g sample of impure CaCO, (s) is dissolved in 50.0 mL of 0.150 M HCl(aq). The equation for the reaction is CaCO,(s) + 2 HCl(aq) — CaCl, (aq) + H, 0(1) + CO2(g) The excess HCl(aq) is titrated by 4.85 mL of 0.125 M NaOH(aq) Calculate the mass percentage of Caco, (s) in the sample. mass percentage: The zinc content of a 1.03 g ore sample was determined by dissolving the ore in HCl, which reacts with the...
Given the following data, calculate the mass percentage of copper in the unknown copper oxide sample...
Given the following data, calculate the mass percentage of copper in the unknown copper oxide sample for this particular trial. Mass of empty test tube: 2.319g Mass of test tube and unknown copper oxide sample: 2.943g Mass of test tube and product (after reaction): 2.630g
How do you calculate grams of H2O2 from the expeimental data given? (acidic medium) MnO4 +...
How
do you calculate grams of H2O2 from the expeimental data given?
(acidic medium) MnO4 + H2O2 = Mn2+ + O2 The spectator ion, K, has been left out of the equation. CH" + 2 MnO4 + Shooa 2M na +502 + 8 H2O BRAND OF HYDROGEN PEROXIDE ANALYZED: If no brand name is provide, create a name for the hydrogen peroxide brand. Be creative. AVERAGE EXPERIMENTAL MOLARITY OF THE KMnO4 SOLUTION USED: 0.0968 M KMnO4 ERLENMEYER FLASK NUMBER: #4...
A sample of copper ore with a mass of 0.4225 g was dissolved in acid. A...
A sample of copper ore with a mass of 0.4225 g was dissolved in acid. A solution of potassium iodide was added, which caused the reaction: 2Cu2+(aq) + 5I– (aq) → I3–(aq ) + 2CuI(s) The I3– that formed reacted quantitatively with exactly 29.96 mL of 0.02100 M Na2S2O3 according to the following equation: I3– (aq) + 2S2O32– (aq) → 3I– (aq ) + S4O62–(aq ) What was the percentage by mass of copper in the ore? If the ore...
c. Given an actual yield of 0.99 g iron(II) oxalate, FeC204.2H20, calculate the percentage yield SO.)...
c. Given an actual yield of 0.99 g iron(II) oxalate, FeC204.2H20, calculate the percentage yield SO.) 6H0+ 2. H.C.O. - fear 2 C-2 - 2 16 FeC20:2H20 +_SH.C.O. + 2 FeC.0, 2H,0 + (NH) SO. + _H.SO. + H0 Fe- 1 0 =15 S=2 H2O2+ 3.KC,8. - K [Fe(COT 3H30 Transfer the balanced chemical reactions to page 6. 4. Use the first of the above balanced chemical equations to determine the following a. The reaction mixture initially contains 2.5 of...
1.) Sodium oxalate, Na2C2O4, in solution is oxidized to CO2(g) by MnO−4 which is reduced to...
1.) Sodium oxalate, Na2C2O4, in solution is oxidized to CO2(g) by MnO−4 which is reduced to Mn2+. A 50.0 −mL volume of a solution of MnO−4 is required to titrate a 0.342 −g sample of sodium oxalate. This solution of MnO−4 is then used to analyze uranium-containing samples. A 4.60 −g sample of a uranium-containing material requires 32.5 mL of the solution for titration. The oxidation of the uranium can be represented by the change UO2+→UO2+2. Calculate the percentage of...
To measure the amount of iron in a certain type of iron ore, an analytical chemist...
To measure the amount of iron in a certain type of iron ore, an analytical chemist dissolves a 24.00 g sample in strong acid and titrates it to the endpoint with 28.8 ml. of 0.4400 M potassium permanganate (KMn0) solution The balanced chemical equation for the reaction is: SH (aq)+SFe (aq) + MnO, (ag) SFe (a)+ Mn(ag) + 4H,0(0 dh Oprecipitation What kind of reaction is this? acid-base X Oredox If you said this was a precipitation reaction, enter the...
Given the following data: C) IT final init (°C) H2O 50.00 ml 21.40 22.28 Na2S203 3.25 g Calculate AHº for the reaction: Na2S2O3(s) - Na2S2O3(aq) You may assume all solutions to have the same density and specific heat as water (1.00 g/mL and 4.184 J/g°C) kJ/mol
calculate tbe hardness of the water given expeirmental data
25
mL of water was used
Part 2: The Hardness of Water Samples Experimental Data Concentration of EDTA O.OLOS N #2-Tap #5- Mineral Sample number #1- Tap # 4-Mineral #3-Mineral 2245 23.10 35.32 33 2 2 34, ss Initial burette reading 19.us 00 43.10 Final burette reading 23.10 22ur Reaction M2 (aq) +EDTA (aq) [M(EDTA) ] (aq) where M2 Ca2 and Mg Calculated Values #1- Tap #5-Mineral #2-Tap #4-Mineral #3-Mineral Volume...
A 0.450 g sample of impure CaCO, (s) is dissolved in 50.0 mL of 0.150 M HCl(aq). The equation for the reaction is CaCO,(s) + 2 HCl(aq) — CaCl, (aq) + H, 0(1) + CO2(g) The excess HCl(aq) is titrated by 4.85 mL of 0.125 M NaOH(aq) Calculate the mass percentage of Caco, (s) in the sample. mass percentage: The zinc content of a 1.03 g ore sample was determined by dissolving the ore in HCl, which reacts with the...
How
do you calculate grams of H2O2 from the expeimental data given?
(acidic medium) MnO4 + H2O2 = Mn2+ + O2 The spectator ion, K, has been left out of the equation. CH" + 2 MnO4 + Shooa 2M na +502 + 8 H2O BRAND OF HYDROGEN PEROXIDE ANALYZED: If no brand name is provide, create a name for the hydrogen peroxide brand. Be creative. AVERAGE EXPERIMENTAL MOLARITY OF THE KMnO4 SOLUTION USED: 0.0968 M KMnO4 ERLENMEYER FLASK NUMBER: #4...
c. Given an actual yield of 0.99 g iron(II) oxalate, FeC204.2H20, calculate the percentage yield SO.) 6H0+ 2. H.C.O. - fear 2 C-2 - 2 16 FeC20:2H20 +_SH.C.O. + 2 FeC.0, 2H,0 + (NH) SO. + _H.SO. + H0 Fe- 1 0 =15 S=2 H2O2+ 3.KC,8. - K [Fe(COT 3H30 Transfer the balanced chemical reactions to page 6. 4. Use the first of the above balanced chemical equations to determine the following a. The reaction mixture initially contains 2.5 of...
To measure the amount of iron in a certain type of iron ore, an analytical chemist dissolves a 24.00 g sample in strong acid and titrates it to the endpoint with 28.8 ml. of 0.4400 M potassium permanganate (KMn0) solution The balanced chemical equation for the reaction is: SH (aq)+SFe (aq) + MnO, (ag) SFe (a)+ Mn(ag) + 4H,0(0 dh Oprecipitation What kind of reaction is this? acid-base X Oredox If you said this was a precipitation reaction, enter the...
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