The tetraethyl lead Pb(C2H5)4 in a 25.00 mL sample of aviation gasoline was shaken with 15.00 mL of 0.02488 M I2. After the reaction was complete, the unused I2 was titrated with 5.39 mL of 0.02670 M thiosulfate solution. Calculate the weight of Pb(C2H5)4 (MW = 323.4 g/mol) in each liter of gasoline.

You are running an acid-base titration with hydrochloric acid and calcium hydroxide.  The calcium hydroxide is your titrant; it has a known concentration of 0.0891 M.  You have added 25.0 mL of the hydrochloric acid solution to an Erlenmeyer flask along with 2 drops of phenolphthalein (fee’-nol-thay-leen) indicator.  To begin your first trial, you fill a clean 50 mL buret with the calcium hydroxide solution.  Your starting volume is 0.25 mL. After the addition of solution from the buret, you see a color change in the flask, and the end point of the reaction is reached.  You note the final volume in the buret to be 18.75 mL. You begin again for your second titration trial.  You add 24.8 mL of the hydrochloric acid solution to a clean flask along with 2 drops of indicator.  You refill the buret to an initial volume of 1.42 mL.  When the reaction is complete, you note the final volume in the buret at 16.74 mL. Then you complete a third trial.  You add 25.6 mL of hydrochloric acid solution…

mare 550 ml of 0,420 M Mg. COH)2 SOlunon?

AaBbCcDdF 三 斗 T AaBbCcDdE AaBbCcAaBbCcDdE Aa v Normal Strong Emphasis Heading 1 v A v 5. What is the maximum amount of water that can be obtained from 22.05 g of copper and 750.00 mL of 1.00 M of nitric acid according to the below reaction? 3 Cu(s) + 8 HNO3(aq) 3 Cu(NO3)2(aq) + 2 NO(g) + 4 H20(t) 6. If 25.00 mL of 2.11x10-8 M Na2SO4 is mixed with 20.00 mL of 1.22x10-8 M Ba(NO3)2, how many grams of precipitate (which is?) can be formed? 7. In all the limiting reactant questions, how much of the excess reactant is left over? Give answer in mass or volume as appropriate. English United States O Focus MacBook Air 吕口 F3 000 FA F2 * ES > F6 F7 FB F9 F10 $4 & 4 6. 7 8 5 III III %#3 |II lili

A sample consisting of Na2CO3 (105.96), NaOH (39.99) and inert matter weighs 1.179 g. It is titrated with 0.300 N HCI with phenolphthalein as the indicator, and the solution becomes colorless after the addition of 48.16 ml. Methyl orange is then added and 24.08 ml more of the acid are needed for the color change. What is the percentage of NaOH and N22CO3? *

Fill in the missing words With the given plot, if a 0.1000 M NaOH solution was used to fully precipitate all the Zn2+ in the form of Zn(OH)2 with the addition of 6.00 mL of NaOH, the number of moles of Zn2+ in this 10 mL brass stock solution is mmol. Therefore, there are mmol of Zn2+ in the entire 100-mL brass stock solution, which is g/mol). mg of Zn2+ (FW = 65

2. The reaction between lead(II) nitrate and potassium iodide solution is shown below   Pb(NO3)2(aq) + 2 KI(aq) → 2 KNO3(aq) + PbI2   Calculate the mass of lead(II) iodide precipitated when 5.00 cm3 of 4.00 mol dm–3 lead(II) nitrate solution  is mixed with 7.50 cm3 of 5.00 mol dm–3 potassium iodide solution.    [Mr / g mol–1: PbI2 = 461.01]

What mass of NaOHNaOH is needed to precipitate the Cd2+ ions from 30.0mL of 0.500 M Cd(NO3)2 solution?

A 25.00 mL aliquot is withdrawn from the liquid portion of saturated Manganese (II) hydroxide and transferred to an Erlenmeyer flask.  After the addition of methyl orange, a titration with 0.0045 M HCl was performed.  The endpoint was reached after 8.72 mL of the acid was added.   What is the balanced chemical equation? How many moles of hydroxide ions were neutralized in the reaction?  What is the molar concentration of hydroxide in the saturated solution?  What is the molar concentration of Magnesium ion in solution?

Potassium hydrogen phthalate (KHPKHP) is often used as a primary standard in acid–base titrations. If 20.05 mL NaOH20.05 mL NaOH is required to neutralize 0.397 g KHP,0.397 g KHP, what is the concentration of the NaOH?