.com/ilrn/takeAssignment/takeCovalentActivity.do?locator-assignment-takeeqeq[Review Topics][References]Calculate the concentration of all ions present in each of the following solutions of strong electrolytes.a. 0.300 mole of Ca (NO3)2 in 400.0 mL of solutionMCa²+ =MNOSb. 5.5 moles of Na2SO4 in 1.25 L of solutionMNa+Submit Answer=40 ° / 4-MMSO₂²-Mc. 3.70 g of NH4 C1 in 390.0 mL of solutionMNH4+MMC =Md. 7.10 g of K3PO4 in 200.0 mL of solutionMK+ =|MMPO4³-MMRetry Entire GroupShow Hint1² st ¹8.009 more group attempts remainingCengage Learning Cengage Technical Supporta♫ hululyf10video

Note : Dear student since you have posted multiple parts question, we will solve only first three…

[Review Topics] Calculate the concentration of all ions present in each of the following solutions of strong electrolytes. a. 0.300 mole of Ca (NO3)2 in 400.0 mL of solution MCa²+ MNO3 M b. 5.5 moles of Na2 SO4 in 1.25 L of solution MNa+= M Mso2 = M c. 3.70 g of NH4 Cl in 390.0 mL of solution M MNH₂+ Mar M d. 7.10 g of K3PO4 in 200.0 mL of solution MK+ = MPO, Submit Answer = = M M M Retry Entire Group 9 more group attempts remaining [References]

[Review Topics] Calculate the concentration of all ions present in each of the following solutions of strong electrolytes. a. 0.300 mole of Ca (NO3)2 in 400.0 mL of solution MCa²+ MNO3 M b. 5.5 moles of Na2 SO4 in 1.25 L of solution MNa+= M Mso2 = M c. 3.70 g of NH4 Cl in 390.0 mL of solution M MNH₂+ Mar M d. 7.10 g of K3PO4 in 200.0 mL of solution MK+ = MPO, Submit Answer = = M M M Retry Entire Group 9 more group attempts remaining [References]

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

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.
1. If 10. g of AgNO3 is available, what volume of 0.40 M AgNO3 solution can be prepared? Volume = mL? 2. A 7.52-g sample of a diprotic acid requires 179.0 mL of a 0.750 M NaOH solution for complete neutralization. Determine the molar mass of the acid. g/mol?
1. What is the molar concentration of Na+ ions in 0.0300 M solutions of the following sodium salts in water? for Na2SO4= Na3PO4= 2. Calculate the final concentrations of the following aqueous solutions after each has been diluted to a final volume of 25.0 mL. for 1.00 mL of 0.470 M Na+ =m 2.00 mL of 3.31 mM LiCl = mM 5.00 mL of 5.95 mM Zn2+ =mM
What volume (mL) of 0.70 M Sodium hydroxide (NaOH) is needed to neutralize 270 mL of 0.40 M Sulfuricacid (H2SO4)?2 NaOH + H2SO4 Na2SO4 + 2 H2O
Gg.168.
1. Write a chemical equation for the dissolution of sodium chloride in water 2. What is the concentration (in moles per litre, mol L−1 or M) of 20.0 g of NaCl in 500.0 mL of distilled water? Show your working. 3. What is the concentration of each of the ions (in moles per litre, mol L−1 or M) in this solution?
50 g of pure Na2CO3 were dissolved in water and the volume of this solution was 200 mL. To this solution, 500 mL of 0.10 M HCl solution were added. Calculate the followings: Moles of Na2CO3 left unreacted Molarity of Na2CO3 solution after the reaction
List the ions and molecules that may have precipitated as part of your final salt product. Step 1. Dissolve the Aluminum metal : (adding solid Al to a Kott Solution) Peaction between Al metal and kot. AICOH and H₂ gas.. Net ionic equation: Solution produces Tetrahydroko aluminate ion 2 A1 (s) + 20H (aq) + 6 +₂0 (1) → 2 Al (OH) - (aq) + 3H2(g) K+(aq) OH(aq) equation that describes the reaction of Sulfuric acid in water: OR H₂SO4 (aq) + H₂0 (1) H₂O+ (aq) + Hs 04" (aq) 2- HSO4 (aq) + H₂O (1) H₂0+ (aq) + 504³ (aq) Step 3: Neutralize base with acid OH reacts with acid: H₂Ocaq) + OH(aq) → 2+1₂0 (1) • Al(OH), reacts with small amount of acid; Alcot)" (q) + Hy" O cag) Al(only (n+ H₂OCD Al(OH) reacts with large amount of acid (with heat): Al (DH), (s) + 3H₂ 0 (aq) → A1 " (aq) + 6 H₂0 (1)
Consider the reaction below: 2 MnO4– + 5 C2O42– + 16 H+ ➜ 2 Mn2+ + 8 H2O + 10 CO2 A 30.0 mL sample of an oxalate solution is found to react completely with 14.5 mL of a 0.1725 M solution of MnO4–. What is the oxalate ion concentration in the sample? Select one: a.0.141 M b.0.033 M c.0.208 M d.0.083 M
11. Solution A was prepared by dissolving 0.60 mol of NaCl in 2.0 L of water. Solution B wa prepared by dissolving 0.60 mol of Na SO4 in 2.0 L of water. What is the concentration of Na ions in solution C which is made by combining equal volumes of solutions A and B. A) 0.30 M B) 0.45 M C) 0.60M D) 0.90 M
12. In a titration of HNO3, you add a few drops of phenolphthalein indicator to 50.00 L if acid in a flask. You quickly add 20.00 mL of 0.0502 M NaOH but overshoot the endpoint, turning the solution a deep pink color. Instead of starting over you add an additional 30.00 mL of the acid, turning the solution colorless. It then takes 3.22 mL of the NaOH to reach the endpoint. a. Write the Molecular, Total Ionic, and Net Ionic Equations for this reaction. b. What is the concentration of the HNO3 solution? c. How many moles of NaOH were in excess after the first addition?
MISSED THIS? Watch IWE: Acid-Base Titration; Read Section 5.7. You can click on the Review link to access the section in your e Text. A 17.00 mL sample of an unknown HClO4 solution requires titration with 17.32 mL of 0.1000 M NaOH to reach the equivalence point. Part A What is the concentration of the unknown HC1O4 solution? The neutralization reaction is HClO4 (aq) + NaOH(aq) → H₂O(1) + NaClO4 (aq) Express the molarity to four significant figures. ► View Available Hint(s) M(HCIO4) = Submit Provide Feedback VE ΑΣΦ VO www ? M Next >