How many milliliters of 0.592 M KOH are needed to react completely with 55.0 mL of 0.271 M FeCl2 solution to precipitate Fe(OH)2? The net ionic equation is: Fe2*(aq) + 20H'(aq) → Fe(OH)2(s) VKOH = i mL

How many milliliters of 0.592 M KOH are needed to react completely with 55.0 mL of 0.271 M FeCl2 solution to precipitate Fe(OH)2? The net ionic equation is: Fe2*(aq) + 20H'(aq) → Fe(OH)2(s) VKOH = i mL

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 95AP: 95. Many metal ions form insoluble sulfide compounds when a solution of the metal ion is treated...

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Distinguish between the terms slightly soluble and weak. electrolyte.
95. Many metal ions form insoluble sulfide compounds when a solution of the metal ion is treated with hydrogen sulfide gas. For example, nickel(II) precipitates nearly quantitatively as NiS when H2S gas is bubbled through a nickel ion solution. How many milliliters of gaseous H2S at STP are needed to precipitate all (he nickel ion present in 10. mL of 0.050 M NiCl2 solution?
Chemistry A sample of NaOH (sodium hydroxide) contains a small amount of Na2CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.100 g of this sample requires 23.98 mL of 0.100 M HCl . An additional 0.700 mL of 0.100 M HCl is required to reach the methyl orange endpoint. What is the percentage of Na2CO3 by mass in the sample? Express your answer to three significant figures and include the appropriate units.
Maganite is the leading brand for antacid to alleviate heartburn. Its active ingredient is a saturated solution of magnesium hydroxide (milk of magnesia) which neutralizes the sudden increase of H+ during heartburn. Its manufacturing company performed microtitration to simulate how the drug works upon intake.A 50.0 mL saturated solution was prepared. After filtering each solution, a 5.0 mL aliquot was transferred to a 25.0 mL Erlenmeyer flask and was titrated using pre-standardized 0.0320 M HCl which resembled the gastric acid. The endpoint was reached after the addition of 52.2 μL titrant.1. What is the concentration of hydroxide ions in the solution? Note: Use the scientific notation of 0.00012 = 1.2e-4 2. Determine s and Ksp of Mg(OH)2.Note: Use the scientific notation of 0.00012 = 1.2e-4
Maganite is the leading brand for antacid to alleviate heartburn. Its active ingredient is a saturated solution of magnesium hydroxide (milk of magnesia) which neutralizes the sudden increase of H+ during heartburn. Its manufacturing company performed microtitration to simulate how the drug works upon intake. A 50.0 mL saturated solution was prepared. After filtering each solution, a 5.0 mL aliquot was transferred to a 25.0 mL Erlenmeyer flask and was titrated using pre-standardized 0.0320 M HCl which resembled the gastric acid. The endpoint was reached after the addition of 52.2 μL titrant. What is the concentration of hydroxide ions in the solution? Determine solubility s.
Adic acid (H2C6H8O4) is an important carboxylic acid compound for the industry in which nylon is manufactured. Adipic acid to be titrated with NaOH according to the following reaction: H2C6H8O4 + 2Na0 -----> 2H2O + Na2C6H8O4 a) Suppose you titrate 0.283g of pure adipic acid, what volume (ml) of 0.1000M NaOH would be needed to reach the equivalence point? b) suppose you do the same titration with 0.304g industrial adipiqje acid (74% w/w). What would be the volume of NaOH required? Please show steps so I will have a better understanding thanks
A student was asked to determine the concentration of ammonia, a volatile substance, in a commercially available cloudy ammonia solution used for cleaning. First the student pipetted 25.00 mL of the cloudy ammonia solution into a 250.0 mL conical flask. 50.00 mL of 0.100 mol L-¹ HCl(aq) was immed added to the conical flask which reactedwith the ammonia in solution. The excess (unreacted) HC1 was then titrated with 21.50 mL 0. 050 M Na2CO3 (aq). Calculate the concentration of the ammonia in the cloudy ammonia solution.
As a technician in a large pharmaceutical research firm, you need to produce 250. mLmL of 1.00 MM potassium phosphate buffer solution of pHpHpH = 6.85. The pKapKa of H2PO4−H2PO4− is 7.21. You have the following supplies: 2.00 LL of 1.00 M KH2PO4M KH2PO4 stock solution, 1.50 LL of 1.00 M K2HPO4M K2HPO4 stock solution, and a carboy of pure distilled H2OH2O. How much 1.00 M KH2PO4M KH2PO4 will you need to make this solution?
You are going to standardize your sodium hydroxide by titrating with potassium hydrogen phthalate. As an example, you dissolve 0.3365 g of potassium hydrogen phthalate, otherwise known as KHP (KHC8H4O4) in water in a 250.0 mL Erlenmeyer flask and then add phenolphthalein indicator. You then titrate with your sodium hydroxide solution, which is in a buret, and you determine that the equivalence point is at 12.44 mL of your sodium hydroxide solution. Determine the molarity of your sodium hydroxide solution. What color will the solution of potassium hydrogen phthalate turn to determine when the equivalence point has been reached?
In standardizing a solution of NaOH (40 g/mol) against 1.431 g of KHP (204.22 g/mol) the analyst uses 35.50 mL of the alkali and has to run back with 8.25 mL of acid (1 mL=10.75 mg NaOH). What is the molarity of the NaOH solution?
A solution of 25 mL Na2CO3 is neutralized with 22.4 mL of 0.1065 M HCl. In the another analysis, 50 mL of Na2CO3 solution is added to 25.0 mL of Pb(NO3)2 solution, and after the lead (II) carbonate was filtrated, the excess of Na2CO3 is neutralized with 14.8 mL of the same acid. According to this, calculate the concentration of lead (II) nitrate (331.2 g/mol) as molarity and g/L?
Hi,can you slove Q.no 1 and Q.no. 2 , all Please. Thank You 1. A student is asked to perform a neutralization reaction between hydrochloric acid, HCl and sodium hydroxide, NaOH. The student transfers 5.00 mL of HCl solution to the titration flask and then adds 25.0 mL of distilled water and 3 drops of phenolphthalein indicator to the solution. The resulting solution uses 35.5 mL of 0.125M NaOH solution to reach the end point.a. Write a balanced chemical equation for the neutralization process.b. What will be the color of solution at the end point?c. Calculate the number of moles of NaOH used for complete neutralization.d. Calculate the strength in terms of molarity for HCl solutione. Calculate the m/v percent strength of the HCl solution 2. If a student calculated that 0.0035 moles of acetic acid present in a 5.0 mL sample of vinegar. Then calculate the mass/volume percent of acetic acid in vinegar