3) A 42.5 ml samples of 0.020 M sulfuric acids is being titrated with 0.050 M ofmagnesium hydroxide. How many milliliters of titrant will be needed to reach theequivalence point?Type of problem?How do you knowWhat are you looking for?What substance do you want and what units do you want it in?Solve4) How many grams of nitrogen can be produced when 26.7 g of ammonia is reacted withexcess oxygen per the following reaction?4NH3(g) + 302(g) → 6 H20(/) + 2N;(g)Type of problem?How do you knowWhat are you looking for?What substance do you want and what units do you want it in?Solve

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3) A 42.5 ml samples of 0.020 M sulfuric acids is being titrated with 0.050 M of magnesium hydroxide. How many milliliters of titrant will be needed to reach the equivalence point? Type of problem? How do you know What are you looking for? What substance do you want and what units do you want it in? Solve

3) A 42.5 ml samples of 0.020 M sulfuric acids is being titrated with 0.050 M of magnesium hydroxide. How many milliliters of titrant will be needed to reach the equivalence point? Type of problem? How do you know What are you looking for? What substance do you want and what units do you want it in? Solve

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Be sure to answer all parts. Radiochemical techniques are useful in estimating the solubility product of many compounds. In one experiment, 50.0 mL of 0.080 M AgNO3 solution containing a silver isotope with a radioactivity of 74,025 counts per min per mL were mixed with 300.0 mL of a 0.040 M NaIO, solution. The mixed solution was diluted to 500.0 mL and filtered to remove all of the AgIO, precipitate. The remaining solution was found to have a radioactivity of 44.4 counts per min per mL.. What is the Ksp of AgIO,? x 10 (Enter your answer in scientific notation.)
The Solubility Product Constant for nickel(II) hydroxide is 2.8 x 10 ^-16 The maximum amount of nickel(II) hydroxide that will dissolve in a 0.130 M nickel(II) nitrate solution is _______M.
Exactly 10.66 ml of 0.066 M strong acid is added to a 30.00 ml. sample of a 0.068 M weak base solution. What is the pH at this point in the titration? K for the base is 2.51x10-5. REPORT YOUR ANSWER TO 2 DECIMAL PLACES. DO NOT INCLUDE UNITS. Type your answer....
An HCl solution has a concentration of 0.09714 M. Then 10.00 mL of this solution was then diluted to 250.00 mL in a volumetric flask. The diluted solution was then used to titrate 250.0 mL of a saturated AgOH solution using methyl orange indicator to reach the endpoint. 1. What is the concentration of the diluted HCl solution? 2. If 7.93 mL of the diluted HCl solution was required to reach the endpoint, what is the concentration of OH− in solution? 3. What is the concentration of Ag+ in solution?
You collected the following data from a titration experiment using a 0.118M standardized NaOH solution to titrate a 26.65 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Find molarity Initial Burette Reading (mL) Final Burette Reading (mL) Vol Delivered (mL) Molarity Trail #1 0.15 19.47 19.32 ?
3
1. How do you prepare a 100mL of 0.1 M phosphate buffer?To make 100 mL of 0.1 M phosphate buffer: Calculate the amount of sodium phosphate needed. moles of sodium phosphate = (0.1 mol/L) x (0.1 L) = 0.01 moles mass of sodium phosphate = moles x molar mass = 0.01 moles x 142 g/mol = 1.42 g Dissolve 1.42 g of sodium phosphate in distilled water in a 100 mL volumetric flask. Adjust the pH of the solution to the desired value (usually around 7.4) using a strong acid or strong base. Bring the solution to the final volume (100 mL) with distilled water. 2. From the anterior buffer, how do you make 100mL of 0.05 M? To make 100 mL of 0.05 M phosphate buffer from the 0.1 M stock solution: Calculate the amount of the 0.1 M phosphate buffer needed. moles of phosphate buffer = (0.05 mol/L) x (0.1 L) = 0.005 moles Calculate the volume of the 0.1 M phosphate buffer needed. moles = concentration x volume (in liters) volume = moles / concentration = 0.005 moles / 0.1 mol/L = 0.05 L or 50 mL Measure…
2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)
moles of NaOH moles moles of acid moles Concentration of acid in original sample in M Volume in mL
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