metal ions! 3+ 2+ 4.35 Water "softeners" remove metal ions such as Caand Fe by replacing them with enough Na ions to maintain the same number of positive charges in the solution. If 1.0x10 L of "hard" water is 0.015 M Ca and 0.0010 M Fe, how many moles of Na are needed to replace these ions? 9 3+ Wising Ecuations for Aqueous lonic Reactions

metal ions! 3+ 2+ 4.35 Water "softeners" remove metal ions such as Caand Fe by replacing them with enough Na ions to maintain the same number of positive charges in the solution. If 1.0x10 L of "hard" water is 0.015 M Ca and 0.0010 M Fe, how many moles of Na are needed to replace these ions? 9 3+ Wising Ecuations for Aqueous lonic Reactions

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

net ion 4
Exchange Reactions (look for 2 soluble salts or a str acid and str base *do not break apart polyatomic ions) 1. NaCl Ag(NO3)3 > Na, (NO3)y Aga Clb What are the subscripts? What is the net ionic + eqn?
3. How many grams of NaOH are needed to prepare 45.0 mL of a 6.00 M solution? 4. What is the molar concentration of 17.5% (v/v) aqueous solution of hydrochloric acid? The density of hydrochloric acid is 1.49 g/mL. Assume the solution is 100.00 mL. 5. What is the concentration of a solution of H₂SO4 if 95.0 mL of a 2.50 M H₂SO4 solution is diluted to a total volume of 275.0 mL? 6. What volume of a 2.28 M aqueous sodium carbonate will completely react with 125 mL of 0.525 M aqueous calcium chloride? 7. 100.0 mL of 0.445 M potassium hydroxide is mixed with 90.0 mL of 0.215 M magnesium nitrate. a. Write the net ionic equation. b. Find the mass of the precipitate in the solution. | c. How many moles of excess reagent will remain at the end of the reaction?
6. A 0.4622-g sample of potassium hyd rogen phthalate was dissolved in 50 mL of deionized water and titrated to a phenolphthalein end-point with 19.48 mL of NaOH solution. What is the molarity of the NaOH? 7. Assuming that the density of vinegar is 1.012 g/m L, calculate the weight percent of acetic acid in vinegar if 23.85 mL of 0.1311 M NaOH was required to titrate 5.00 mL of vinegar. did HA nd dis 192 riw o asuuc no'noleauoetb s obulbo. As 900 900 4Coz2 anigll .asbtucf namheqx dini 209 (0 HoO Cag) (es) ibis 9C D DV 9 ballet tnabole A 9 u u 1oied qütenud orlf hi asiddud e 9t borsoog szib alddud sis ord nolt dsvawnlcrndtuodA 9l il blucwnolduloe HOe wans uoy nistqx3 Sipid oo! tstse : wot oo dhelom t bbs rg beau yilednobbos nsbile s est itbin ow osta isrl bsbne evicmi Srtulce HOs orts to yahelom orld ininetsb as 9 adant anoto toi n odslo 613 Exbiont Aorf
5. A student conducted a titration experiment. He/she used 12.0 mL of silver nitrate (titrant) solution to reach the endpoint. If the student used 25.4 mL of the chloride (analyte) for the titration and found the concentration of chloride ions to be 2.2 M, what is the mass (in grams) of silver nitrate titrant Clic)
to 70 ml of 0.2M Pb solution (NO3) 2 add 30 ml of 0.7 M KIO3 solution. a) Write the equation of the chemical reaction and calculate the number of moles of Pb2 + and IO3- ions before mixing b) count the number of moles of Pb2 + and IO3- ions after mixing, knowing that Ksp of Pb (IO3) 2 = 2.5 × 10-¹³
In a double replacement precipitation reaction, KCl reacts with Pb(NO3)2 in a 2:1 mole ratio, respectively. Calculate the volume in mL of a 0.100 mol/L Pb(NO3)2 solution needed to completely react with 40.0 mL of a 0.500 mol/L solution of KCl?
solution after precipitation is complete. 68. The drawings below represent aqueous solutions. Solution A is 2.00 L of a 2.00-M aqueous solution of copper(II) nitrate. Solution B is 2.00 L of a 3.00-M aqueous solution of potas- sium hydroxide. (0) suiro Cu²+ ebro NO3 БО K+ OH™ A B a. Draw a picture of the solution made by mixing solutions A and B together after the precipitation reaction takes place. Make sure this picture shows the correct relative volume compared to solutions A and B, and the correct relative number of ions, along with the correct relative amount of solid formed. b. Determine the concentrations (in M) of all ions left in solution (from part a) and the mass of solid formed.
100 mL of water contain 100 mg of strontium Sr²+. What mass of solid potassium chromate K2 CrO4 should be added to this solution to precipitate 99% of the strontium contained in the solution? The only possible reaction is the precipitation of strontium chromate, SrCrO4. 87.6 g.mol-¹; KSrCrO4 = 3×10−5 Data: MK₂CrO4 194.2 g.mol-¹; Msr The answer : m 5.33 g = -
Question 9 of 21 > O Macmillan Learning You decide it is time to clean your pool since summer is quickly approaching. Your pool maintenance guide specifies that the chlorine, Cl₂, concentration of the pool should be between 1 and 3 ppm. In order to determine if your pool is safe to swim in, you send a sample of pool water to a chemist for analysis of the Cl₂ content. The chemist reports a chlorine concentration of 3.92 × 10-5 M. Convert the concentration of Cl₂ to parts per million (ppm). concentration: 2.71 Incorrect Attempt 3 ppm
4. Calculate the calculate the mass of precipitate formed from 5.0 g of strontium chloride. Li3PO4(aq) → Sr3(PO4)2(S) + LiCl(aq) _SrCl₂(aq) + 5. What mass of aluminum hydroxide in needed to neutralize 5.00 g of hydrochloric acid? Al(OH)3(s) + _HCl(aq) → ___AlCl3(aq) + _H₂O(1) 195
If 0.468 L of water is added to a 59.1 mL of 17.2 M stock solution of acetic acid (CH 3COOH), what is the resulting concentration?