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

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...

See similar textbooks

Similar questions

The concentration of SO42– ions in a 45.0 mL sample of seawater is determined by adding a solution of BaCl2 and precipitating the SO42– as BaSO4. After the precipitate is filtered from the solution, it is dried and weighed. If the mass of BaSO4 recovered is 0.315 g, what is the sulfate concentration of the seawater sample? Express your answer in mmol/L.
Through this reaction HCl(aq) + NaHCO3(aq)— NaCl(aq) +H2O(l) +CO2(g). The CO2 gas produced is what makes you burp. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 100. mL of a 0.092 M HCl solution. What mass of NaHCO would he need to ingest to neutralize this much HCl? Round your answer to 2 significant digits
The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated as KHP). KHP is an acid with one acidic hydrogen and a molar mass of 204.22 g/mol. In the titration, 62.32 mL of the sodium hydroxide solution was required to react with 0.5250 g KHP. Calculate the molarity of the sodium hydroxide. Molarity = ____ M
Write the net ionic equation, including phases, that corresponds to the reaction Pb(CIO,),(aq) + K,CO,(aq) → PbCo, (s) + 2 KCIO, (aq) net ionic equation:
The traditional method of analysis for the amount of chloride ion present in a sample is to dissolve the sample in water and then slowly to add a solution of silver nitrate. Silver chloride is very insoluble in water, and by adding silver nitrate, it is possible effectively to remove all chloride ion from the sample. Ag+(aq) + Cl-(aq) → AgCl(s) Suppose a 1.515 g sample is known to contain 27.5% chloride ion by mass. What mass of silver nitrate must be used to completely precipitate the chloride ion from the sample?
In a laboratory experiment, a 19.0 −mL−mL sample of KClKCl solution is poured into an evaporating dish with a mass of 24.60 gg . The combined mass of the evaporating dish and KClKCl solution is 43.50 gg . After heating, the evaporating dish and dry KClKCl have a combined mass of 29.93 g What is the molarity (M) of the KCl solution?
In a titration experiment, a 5.00-mL sample of sulfuric acid, H2SO4, from a car battery is diluted with de-ionized water to 100.0 mL. A 20.00-mL portion of the diluted acid is titrated with 0.2025 MNaOH solution. If 42.00 mL of the NaOH solution is required to neutralize the dilute acid, what is the molar concentration of H2SO4 in the original solution taken from the battery? The acid-base reaction occurs as follows: H2SO(aq) + 2NaOH(aq) --> Na2SO4(aq) + 2H2O(l) (A) 0.2126 M (B) 0.4252 M (C) 4.25 M (D) 8.50 M
1. (a) Write balanced molecular equations for the following potential precipitation reactions. Indicate the states of reactants and products [(aq) or (s)]. (b) In those cases where a precipitate forms, write the net ionic equation. If there is no reaction, state "No reaction." (i) NiCl₂ (aq) + K₂S (aq) → (iii) NH4Cl (aq) + Pb(NO3)2 (aq) →→ (ii) MgCl₂ (aq) + Cu(NO3)2 (aq) → (iv) FeSO4 (aq) + Na3PO4 (aq) →
How many grams of Cu(OH)2 will precipitate when excess KOH solution is added to 41.0 mL of 0.618 M CuBr2 solution? CuBr2(aq) + 2KOH(aq) Cu(OH)2(s) + 2KBr(aq)g?
Classify each of these reactions. 2 NaOH(aq)+Pb(CI0,),(aq)- → 2 NACIO, (aq)+Pb(OH),($) CH,(g) + 20,(g) → CO,(g) + 2 H,0(1) 2 AGNO, (aq)+Zn(s) • Zn(NO, ),(aq) + 2 Ag(s) HI(aq)+L¡OH(aq) – H,O(1)+Lil(aq) Answer Bank precipitation acid base neutralization redox
Two solutions were made, the first one was made by dissolving 2.27 g of Co(NO3)2 in 100.0 mL of water. Then, to make the second solution, 5.00 mL of this solution was added to the 250 mL volumetric flask, which was filled to the mark with water. What was the molar concentration of the Co(NO3)2 in the two solutions?
A volume of 10 mL of an unknown hydrochloric acid sample was diluted to 100 mL. The diluted solution was then titrated against a solution of sodium carbonate (prepared by dissolving 0.2188 g of solid in 50 mL distilled water). Hydrochloric acid reacted with sodium carbonate according to the following equation: 2 HCI (aq) + Na,CO3 (aq)H20 () + CO2 (g) + 2 NaCl (aq) A volume of 15.2 mL of the hydrochloric acid was required to complete the reaction in the titration process. A second titration was done between the same acid sample against a blank for indicator correction, a volume of 0.3 mL was consumed by the indicator. Find the moles of HCI added and concentration of dilute HCI solution. [MM of Na CO3 = 105.99 g/mol, MM of HCI = 36.46 g/mol] 2.06x10-3 mol ; 0.277 M B 2.06 x10-3 mol; 0.135 M 4.13x10-3 mol ; 0.277 M 4.13x10-3 mol ; 0.272 M