13. (d) Pharmacists sell tablets containing magnesium hydroxide, Mg(OH),, to combat indigestion. A student caried out an investigation to find the percentage by mass of Mg(OH), in an indigestion tablet. The student reacted the tablet with dilute hydrochloric acid. Mg(OH),(s) + 2HC{aq) → MgCL(aq) + 2H,0() The student found that 32.00 cm³ of 0.500mol dm 3 HClwas needed to react with the Mg(OH)2 in a 500 mg tablet. [1g = 1000 mg]. (i) Calculate the amount, in mol, of HCL used. mol amount = (i) Determine the amount, in mol, of Mg(OH), present in the tablet. amount = mol (iii) Determine the percentage by mass of Mg(OH), present in the tablet. answer =

13. (d) Pharmacists sell tablets containing magnesium hydroxide, Mg(OH),, to combat indigestion. A student caried out an investigation to find the percentage by mass of Mg(OH), in an indigestion tablet. The student reacted the tablet with dilute hydrochloric acid. Mg(OH),(s) + 2HC{aq) → MgCL(aq) + 2H,0() The student found that 32.00 cm³ of 0.500mol dm 3 HClwas needed to react with the Mg(OH)2 in a 500 mg tablet. [1g = 1000 mg]. (i) Calculate the amount, in mol, of HCL used. mol amount = (i) Determine the amount, in mol, of Mg(OH), present in the tablet. amount = mol (iii) Determine the percentage by mass of Mg(OH), present in the tablet. answer =

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section: Chapter Questions

Problem 120QRT

See similar textbooks

Similar questions

Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman Empire can be traced, in part, to high levels of lead in water from containers and pipes, and from wine that was stored in leadglazed containers. If we presume that the typical Roman water supply was saturated with lead carbonate, PbCO3 (Ksp = 7.4 1014), how much lead will a Roman ingest in a year if he or she drinks 1 L/day from the container?
6-40 What is the molarity of each solution? (a) 47 g of KCI dissolved in enough water to give 375 mL of solution (b) 82.6 g of sucrose, C12H22O11, dissolved in enough water to give 725 mL of solution (c) 9.3 g of ammonium sulfate, (NH4)2SO4 dissolved in enough water to give 2.35 L of solution
Q1. A solution was prepared by dissolving 1210 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 775 mL. Calculate (a) the molar analytical concentration of K-Fe(CN)6- (b) the molar concentration of K+. (c) the molar concentration of Fe(CN) (d) the weight/volume percentage of K3Fe(CN)6. (e) the number of millimoles of K1 in 50.0 mL of this solution. (f) ppm Fe(CN)6¹
3 Bal, (aq)+ 2 Nag POq Caq) 7 BalPO42 + l6 Nal laq • Consider the reaction of 30.0mL of 0.270M Balz with 20.0 mL of 0.3ISM Naz PO4. Lwhat quantity in meles of Balz are preset in the solution? are produced /What quantitg in moles of precipitate E ali Bal were consumed based on the balanced chomical equation? 6) What auantity in males of Na3 Pla aro present in soluction? d) What quantity in moles of precipitate are paduced if all the Naz PO, were cansumed based on the balanced chemi.cal equation? e) which reactant is limisting f What mass (in g) of precipitate is firemed when the limiting reactant is considered?
1-1. The raw water supply for a community contains 18 mg/L total particulate matter. It is to be treated by addition of 60 mg alum (Al2(SO4)3-14H;O) per liter of water treated. Essentially, all the added alum precipi- tates represented by the following reaction: Al2(SO4)3 · 14H20 → 2 Al(OH);(s) + 3So,- + 6H* + 8H2O For a total flow of 7500 m/d, compute the daily alum requirement, the total concentration of suspended sol- ids in the water following alum addition, and the daily load of particulate solids requiring disposal (including both those initially present and those formed during treatment).
*4-33. Exactly 0.2220 g of pure Na₂CO3 was dissolved in 100.0 mL of 0.0731 M HCL. (a) What mass in grams of CO₂ were evolved? (b) What was the molarity of the excess reactant (HCI or Na₂CO,)?
nedtrcl (7Jon the PH Fepes. 6. The concentration of a sulfuric acid solution isn't known, so it's titrated with an aqueous solution containing 3.00 g of sodium hydroxide. It took 22.8 mL of sulfuric acid solution to neutralize the base. a) Write a balanced equation (with phases) for the reaction that's taking place. b) How many moles of sodium hydroxide were present? c) How many moles of sulfuric acid must have been present? d) What is the concentration of the acid solution?
2-12. What is the mass in milligrams of solute in (a) 26.0 mL of 0.150 M sucrose (342 g/mol)? (b) 2.92 L of 5.23 X 10-3 M H,O2?
2 Analytical Chemi... -> Analytical Chemistry Problems Q1/ What is the weight, in milligrams, of 0.250 mmol Fe2O3 (ferric oxide), F.wt (159.7 mg/mmol)? Q2/ A solution is prepared by dissolving 1.26 g AGNO3 in a 250-mL volumetric flask and diluting to volume. Calculate the molarity of the silver nitrate solution. How many millimoles AGNO3 were dissolved? F.wt AGNO3 169.9 g/mol Q3/ How many grams per milliliter of NaCl are contained in a 0.250 M solution? F.wt NaCI 58.4 mg/mmol Q4/ Calculate the concentration of potassium ion in grams per liter after mixing 100mL of 0.250 M KCI and 200mL of 0.100 M K2SO4. (atomic weight K 39.1 mg/mmol) Q5/ How many milliliters of concentrated sulfuric acid, 94.0%, density 1.831 g/cm3, are required to prepare 1 liter of a 0.100 M solution? F.wt H2SO4 98.1 g/mol Q6/ You wish to prepare 500mL of a 0.100 M K2Cr2O7 solution from a 0.250 M solution. What volume of the 0.250 M solution must be diluted to 500 mL? Q7/ The concentration of zinc ion in blood serum…
C0 96 Gran The Rate of a Reaction Table of Content and Preface prod.mheducation.com/epub/sn_7e4a4/data-uuid-326b493dfd7f46f3b7d174cd33673180 + X Price vs Kes. O Stanton Iron Canop... 6 Stanton Iron Canop.. Dental Health Servi. O Vitamins | Supplem.. S https://ezto.mhedu. Duke Energy Example 14.1 Write the rate expressions for the following reactions in terms of the disappearance of the reactants and the appearance of the products: (a) I¯ (aq) + OCI" (aq) → Cl¯ (aq) + OI (aq) (b) 302 (g) → 203 (g) (c) 4NH3 (g) + 502 (g) → 4NO (g) + 6H2O (g) Solution (a) Because each of the stoichiometric coefficients equals 1, [_I] V At A [OCI¯] rate = %3D At [_I0] V (b) Here the coefficients are 3 and 2, so [0]v I 2 At 1 A[O3] rate = %3D 3. (c) In this reaction 91 /口因 OL pause break prt sc sysrq delete nsect %24 9. 7. P. H B. W N 1 ɔ
Using the average molarity of the NaOH solution determined from your results in part A, calculate the molarity and percent by mass of the acetic acid in your vinegar sample and report their average values. H2C2O4•2H2O(s) + 2NaOH (aq)= Na2C2O4 + 4H2O(l) part A Mass of oxalic acid analyzed (g)- trial 1- 0.302 trial 2- 0.305 initial buret reading of NaOH (mL)- trial 1-0.31 trial 2- 23.42 final buret reading of NaOH (mL) trial 1- 23.42 trial 2 -46.73 Part B volume of vinegar analyzed (mL), trial 1- 5.00 , trial 2- 5.00 initial buret reading of NaOH (mL), trial 1 -0.00, trial 2 - 22.73 final buret reading of NaOH (mL) trial 1- 22.73, trial 2- 45.50 There is no molarity of oxalic acid that was used during the experiment given
6-17. A 0.3396-g sample that assayed 96.4% Na,SO4 re- quired 37.70 mL of a barium chloride solution. Reaction: Ba2+ + SO- → BaSO,(s) Calculate the analytical molarity of BaCl, in the so- lution.