I need help plotting the mass of precipitate versus moles of Pb(NO3)2 .
Reaction Equation: Pb(NO3)2 + 2KBr → PbBr2 + 2KNO3
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I need help plotting the mass of precipitate versus moles of
Pb(NO3)2 .
Reaction Equation: Pb(NO3)2...
Plot 1 Mass of precipitate (8) 0.002 0.008 0.01 0.004 0.006 Moles of Pb(NO3)2 Plot 2...
Plot 1 Mass of precipitate (8) 0.002 0.008 0.01 0.004 0.006 Moles of Pb(NO3)2 Plot 2 Mass of precipitate (g) 0.002 0.008 0.01 0.004 0.006 Moles of KBr Given the plots provided, estimate the following: The number of moles of Pb(NO3)2 that produce a balanced stoichiometry for the reaction. 0.003 0.004 O 0.006 O 0.008
Consider the balanced equation of KI reacting with Pb(NO3)2 to form a precipitate. 2KI(aq)+Pb(NO3)2(aq)⟶PbI2(s)+2KNO3(aq) What mass...
Consider the balanced equation of KI reacting with Pb(NO3)2 to form a precipitate. 2KI(aq)+Pb(NO3)2(aq)⟶PbI2(s)+2KNO3(aq) What mass of PbI2 can be formed by adding 0.413 L of a 0.140 M solution of KI to a solution of excess Pb(NO3)2?
i need help with questions for part b only please ZULU Acid-Base Titration (worksheet to be...
i need help with questions for part b only please
ZULU Acid-Base Titration (worksheet to be completed in pairs - dee via e-mail Thursday, April 2, 11:59 pm) Concentration of NaOH: 0.0993 mol/L Part A: The following data was obtained when a 20.00 mL sample of acetic acid was titrated with 0.0993 mol/L sodium hydroxide (NaOH). The indicator changed color when 18.90 mL of NAOH was added (highlighted below). pH pH Volume of Base (mL) 1.00 2.00 Volume of Base...
Following the Procedure of this experiment, a student titrated 0.653 g of an unknown weak, monoprotic...
Following the Procedure of this experiment, a student titrated 0.653 g of an unknown weak, monoprotic acid with 0.100 M NaOH and monitored the titration with a pH meter. His titration data were: Volume of NaOH solution added, mL /// pH 0.00 | 3.30 2.00 | 4.22 4.00 | 4.55 6.00 | 4.76 8.00 | 4.92 10.00 | 5.06 12.00 | 5.18 14.00 | 5.29 16.00 | 5.40 18.00 | 5.51 20.00 | 5.62 22.00 | 5.74 24.00 | 5.88...
pH be at the equivalence point? Volume NaOH added pH 0.39 The student collected the following...
pH be at the equivalence point? Volume NaOH added pH 0.39 The student collected the following data: Plot the data above in excel with pH values on the Y axis and the volume of NaOH added on the X axis Graphically determine the equivalence point and indicate the pH on the graph. b. 0.00 2.00 4.00 0.46 0.54 ii. 0.62 6.00 8.00 10.00 0.7 0.78 Show the following calculations on a separate sheet of paper: 0.87 12.00 0.96 1.07 14.00...
A 3.10-g sample of lead nitrate, Pb(NO3)2, molar mass = 331 g/mol, is heated in an...
A 3.10-g sample of lead nitrate, Pb(NO3)2, molar mass = 331 g/mol, is heated in an evacuated cylinder with a volume of 2.00 L. The salt decomposes when heated, the unbalanced equation for the decomposition reaction is shown below: Pb(NO3)2(s) → PbO(s) + NO2(g) + O2(g) Assuming complete decomposition, what is the pressure in the cylinder after decomposition and cooling to a temperature of 303 K? Assume the PbO(s) takes up negligible volume.
Enter the following data into the calculator and graph pH versus mL of NaOH added. At...
Enter the following data into the calculator and graph pH versus mL of NaOH added. At the endpoint you should see a rapid change in pH. Identify the two volumes on each side of the endpoint, and determine the color change of the indicator for the end point. Data Analysis Table Volume of NaOH Solution Added pH Color 0.00 mL 2.79 Clear 1.00 mL 3.99 Magenta then clear 2.00 mL 4.49 Magenta then clear 3.00 mL 4.99 Magenta then clear...
please help with question 3 part b on the first picture? please step by step explain...
please help with question 3 part b on the first picture?
please step by step explain thank you
he leo the acid 3. Following the Procedure of this experiment, a student monoprotic acid with 0.100M NaOH and monitored the titration with a pH meter. His titration titrated 0.653 g of an unknown weak, monoprotic acid with data were: volume of NaOH solution added, mL volume of NaOH solution added, mL pH 0.00 2.00 4.00 6.00 3.30 22.00 24.00 26.00 28.00...
5) Choose the best classification of the reaction represented by the following equation: Pb(NO3)2(ay)+CaClg(ay)-PbCl20)+ Ca(NO3)2(a) A)...
5) Choose the best classification of the reaction represented by the following equation: Pb(NO3)2(ay)+CaClg(ay)-PbCl20)+ Ca(NO3)2(a) A) decomposition B) precipitation C) oxidation-reduction D) acid-base E) combustion 5) 6) 6) Choose the best classification of the reaction represented by the following equation: HBr(ay)+ KOH(ag)KBr(ag) + H20( A) acid-base B) precipitation C) combustion D) combination E) decomposition 7) 7) Magnesium hydroxide, Mg(OH)2, as "Milk of Magnesia" can be used to neutralize excess stomach acid, represented by HCl(ag) according to the chemical equation below....
Monitosing.Acid-Base Titrations wih a pH Meter 3. student titrated 20.0 mL of 0.410M HCI with 0.320M...
Monitosing.Acid-Base Titrations wih a pH Meter 3. student titrated 20.0 mL of 0.410M HCI with 0.320M NaOH and collected the following data. Pre-Laboratory Assignment 1. Briefly explain: (a) why you must use caution when with HCI solutions 0.32 A working volume NaOH solution added, mLpH 0.39 0.46 0.54 0.62 0.70 0.78 0.87 0.96 1.07 1.19 1.35 1.56 1.93 2.09 2.35 3.06 11.40 11.80 12.00 12.20 12.30 0.00 2.00 4.00 6.00 8.00 10.00 12.00 14.00 16.00 18.00 20.00 22.00 24.00 24.50...
Plot 1 Mass of precipitate (8) 0.002 0.008 0.01 0.004 0.006 Moles of Pb(NO3)2 Plot 2 Mass of precipitate (g) 0.002 0.008 0.01 0.004 0.006 Moles of KBr Given the plots provided, estimate the following: The number of moles of Pb(NO3)2 that produce a balanced stoichiometry for the reaction. 0.003 0.004 O 0.006 O 0.008
i need help with questions for part b only please
ZULU Acid-Base Titration (worksheet to be completed in pairs - dee via e-mail Thursday, April 2, 11:59 pm) Concentration of NaOH: 0.0993 mol/L Part A: The following data was obtained when a 20.00 mL sample of acetic acid was titrated with 0.0993 mol/L sodium hydroxide (NaOH). The indicator changed color when 18.90 mL of NAOH was added (highlighted below). pH pH Volume of Base (mL) 1.00 2.00 Volume of Base...
pH be at the equivalence point? Volume NaOH added pH 0.39 The student collected the following data: Plot the data above in excel with pH values on the Y axis and the volume of NaOH added on the X axis Graphically determine the equivalence point and indicate the pH on the graph. b. 0.00 2.00 4.00 0.46 0.54 ii. 0.62 6.00 8.00 10.00 0.7 0.78 Show the following calculations on a separate sheet of paper: 0.87 12.00 0.96 1.07 14.00...
please help with question 3 part b on the first picture?
please step by step explain thank you
he leo the acid 3. Following the Procedure of this experiment, a student monoprotic acid with 0.100M NaOH and monitored the titration with a pH meter. His titration titrated 0.653 g of an unknown weak, monoprotic acid with data were: volume of NaOH solution added, mL volume of NaOH solution added, mL pH 0.00 2.00 4.00 6.00 3.30 22.00 24.00 26.00 28.00...
5) Choose the best classification of the reaction represented by the following equation: Pb(NO3)2(ay)+CaClg(ay)-PbCl20)+ Ca(NO3)2(a) A) decomposition B) precipitation C) oxidation-reduction D) acid-base E) combustion 5) 6) 6) Choose the best classification of the reaction represented by the following equation: HBr(ay)+ KOH(ag)KBr(ag) + H20( A) acid-base B) precipitation C) combustion D) combination E) decomposition 7) 7) Magnesium hydroxide, Mg(OH)2, as "Milk of Magnesia" can be used to neutralize excess stomach acid, represented by HCl(ag) according to the chemical equation below....
Monitosing.Acid-Base Titrations wih a pH Meter 3. student titrated 20.0 mL of 0.410M HCI with 0.320M NaOH and collected the following data. Pre-Laboratory Assignment 1. Briefly explain: (a) why you must use caution when with HCI solutions 0.32 A working volume NaOH solution added, mLpH 0.39 0.46 0.54 0.62 0.70 0.78 0.87 0.96 1.07 1.19 1.35 1.56 1.93 2.09 2.35 3.06 11.40 11.80 12.00 12.20 12.30 0.00 2.00 4.00 6.00 8.00 10.00 12.00 14.00 16.00 18.00 20.00 22.00 24.00 24.50...
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