3. Which of the following statement/s is/are correct?I. 6.00 N H2C0, is equivalent to 3.00M H2CO3.II. 5.29 % (w/v) H2SO, is equivalent to 0.539 N H,SO.III. 1.15 N Mg(OH2 is equivalent to 16.3 g Mg(OH), in 500 mL solution.(MH2S04 - 98.086 g/mol; M2c03 - 62.026 g/mol: MvgOH2-58.326 g/mol)%3DO l and IIO lonlyAl and IlIOHand It

Normality = Molarity * No of H+ ions Molarity = No of moles / Volume (L) No of moles = Mass / Molar…

3. Which of the following statement/s is/are correct? I. 6.00 N H2CO3 is equivalent to 3.00M H2CO3. II. 5.29 % (w/v) H2SO, is equivalent to 0.539 N H2SO. III. 1.15 N Mg(OH)2 is equivalent to 16.3 g Mg(OH), in 500 mL solution. (MH2S04 = 98.086 g/mol; MH2C03 - 62.026 g/mol: MMgOH2 = 58.326 g/mol) !! O I and II Olonly Ol and IlI OHand II

3. Which of the following statement/s is/are correct? I. 6.00 N H2CO3 is equivalent to 3.00M H2CO3. II. 5.29 % (w/v) H2SO, is equivalent to 0.539 N H2SO. III. 1.15 N Mg(OH)2 is equivalent to 16.3 g Mg(OH), in 500 mL solution. (MH2S04 = 98.086 g/mol; MH2C03 - 62.026 g/mol: MMgOH2 = 58.326 g/mol) !! O I and II Olonly Ol and IlI OHand II

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 88QAP

See similar textbooks

Similar questions

The freezing point of 0.10 M KHSO3 is -0.38C. Which of the following equations best represents what happens when KHSO3 dissolves in water? (a) KHSO3(s)KHSO3(aq) (b) KHSO3(s) K+(aq)+HSO3(aq) (c) KHSO3(s) K+(aq)+SO32(aq)+ H+(aq)
The freezing point of a 0.11 m solution of HNO2 is -0.20C. (a) What is i for the solution? (b) Is the solution made (i) of HNO2 molecules only? (ii) of H+ and NO2- only? (iii) of more HNO2 molecules than H+ ions? (iv) primarily of H+ and NO2- ions with some HNO2 molecules?
A patient has a “cholesterol count” of 214. Like manyblood-chemistry measurements,this result is measured inunits of milligrams per deciliter (mgdL1). Determine the molar concentration of cholesterol inthis patient’s blood, taking the molar mass of cholesterolto be 386.64gmol1. Estimate the molality of cholesterol in the patient’sblood. If 214 is a typical cholesterol reading among men inthe United States, determine the volume of such bloodrequired to furnish 8.10 g of cholesterol.
A solution is made by dissolving 0.455 g of PbBr2 in 100 g of H2O at 50C. Based on the data in Table 8-1, should this solution be characterized as a. saturated or unsaturated b. dilute or concentrated
A solution is made by dissolving 34.0 g of NaCl in 100 g of H2O at 0C. Based on the data in Table 8-1, should this solution be characterized as a. saturated or unsaturated b. dilute or concentrated
The Henry's law constant for the solubility of argon gas in water is 1.0103M/atm at 30C. (a) Express the constant in M/mm Hg. (b) If the partial pressure of argon gas at 30C is 693 mm Hg, what is the concentration (in M) of the dissolved argon gas at 30C? (c) How many grams of argon gas can be dissolved in 29 L of water at 693 mm Hg and 30C? (Ignore the partial pressure of water.)
The freezing point of a 0.21 m aqueous solution of H2SO4 is -0.796C. (a) What is i? (b) Is the solution made up primarily of (i) H2SO4 molecules only? (ii) H+ and HSO4- ions? (iii) 2H+ and 1SO42- ions?
Insulin is a hormone responsible for the regulation of glucose levels in the blood. An aqueous solution of insulin has an osmotic pressure of 2.5 mm Hg at 25C. It is prepared by dissolving 0.100 g of insulin in enough water to make 125 mL of solution. What is the molar mass of insulin?
6-38 Describe how we would prepare 250 mL of 0.10 M NaOH from solid NaOH and water.
Epinephrine (or adrenaline) is a hormone and neurotransmitter. It participates in the fight-or-flight response of the sympathetic nervous system. An aqueous solution of epinephrine is prepared by dissolving 0.250 g of the hormone in enough water to make 0.350 L of solution. The solution has an osmotic pressure of 71.8 mm Hg at 22C. What is the molar mass of epinephrine?
Solutions Introduced directly into the bloodstream have to be isotonic with blood; that is, they must have the same osmotic pressure as blood. An aqueous NaCl solution has to be 0.90% by mass to be isotonic with blood. What is the molarity of the sodium ions in solution? Take the density of the solution to be 1.00 g/mL.
6-39 Assuming that the appropriate volumetric flasks are available, describe how we would make these solutions: (a) 175 mL of a 1.14 M solution of NH4Br in water (b) 1.35 L of a 0.825 M solution of Nal in water (c) 330 mL of a 0.16 M solution of ethanol, C2H6O, in water