1. Circle the compounds below that will dissociate to give ions in water (Hint: think which one will give ions insolution. lonic compound ionize - what about HCI?)NaNO,CH,HCIKCI2. For the compounds above, write which will be an electrolyte3. Write the equation that shows dissociation and the ions produced in the following compounds.■. CaSb. Na.SO,=c. Al(SO),4. Which of the following compounds are acids and which are bases? And which is neither?NaOHNaNO,H,PO,NH,OHHNO,5. Look at the solubility guidelines and predict if the following compounds will be soluble in water.PbSO,каCasAgClNaNO,Mg(OH)₂6. Write the molecular, ionic and net ionic equation for the reaction between copper (II) sulfate and bariumchloride.Molecular:Ionic:Net Ionic:

According to the guidelines we are asked to solve only the first 3 subparts. Please post other…

1. Circle the compounds below that will dissociate to give ions in water (Hint: think which one will give ions in solution. Ionic compound ionize - what about HCI?) HCI KCI NaNO, CH, 2. For the compounds above, write which will be an electrolyte 3. Write the equation that shows dissociation and the ions produced in the following compounds. ■ Cas b. Na.SO, = c. Al(SO),

1. Circle the compounds below that will dissociate to give ions in water (Hint: think which one will give ions in solution. Ionic compound ionize - what about HCI?) HCI KCI NaNO, CH, 2. For the compounds above, write which will be an electrolyte 3. Write the equation that shows dissociation and the ions produced in the following compounds. ■ Cas b. Na.SO, = c. Al(SO),

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...

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11. Complete and balance each of the following equations. Use the activity series and solubility table when necessary. COMBINATION REACTIONS a. H2 + Br2 ------ ? c. Na + Cl2 ------ ? d. Nitrogen gas + oxygen gas -------- nitrogen dioxide h. PbCl2 ---- ? + ? j. Zinc + sulfuric acid ------------ ? + ? k. Ni + Al(NO3) 3 -------- ? + ? l. Al + Hg(C2H3O2)2 --------- ? + ? m. Sulfuric acid + ammonium hydroxide ---------- ? + ? n. Silver nitrate + barium chloride ----------- ? + ? p. NaNO 3(aq) + KCl(aq) --------- ? + ? ▼23. Balance each of the following reactions and determine which substance is oxidized and which is reduced: a. K + Cl 2 ------KCI b. NH3 ---- N2 + H2 c. CuO + H2 ----- Cu + H2O d. Sn + Cl 2 ------ SnCl 4
Given equimolar amounts of these solids in separate beakers of distilled water, which one would result to the brightest light bulb in the conductivity test? a. KOH(s) b. BaCO3 c. Ca(OH)2 d. Al(NO3)3
only question number 1 please complete
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?
please answer this question, ignore the writing under
With respect to the following solutes in aqueous solution, I. methane, CH4 II. methanol, CH3OH III. barium nitrate, Ba(NO3)2 IV. hydrofluoric acid, HF V. potassium chloride, KCl which of the following statements is true? Select one: a. These are all strong electrolytes. b. Only III and V are strong electrolytes. c. These are all weak electrolytes. d. I is a weak electrolyte; II, III, IV and V are strong electrolytes. e. Only V is a strong electrolyte.
An aqueous solution of ammonium sulfide is mixed with an aqueous solution of iron (III) Chloride. a. Write a balanced molecular equation, complete ionic equation, and net ionic equation for the two solutions mixed above. Include all phases. b. If 50.0 mL of 0.5(X) M ammonium sulphide and 100.0 mL of 0.250 M iron (III) chloride arc mixed, how many grams of precipitate will form? c. What are the concentrations of ammonium ion and iron (III) ion left in solution after the reaction is complete? d. In part b, you started with 100.0 mL of 0.250 M iron chloride. How would you prepare such a solution in the lab if you started with solid iron(III) chloride?
8.
15. Select the correct statements below. Table salt is a good conductor of electricity because it is a strong electrolyte Table sugar is a weak conductor of electricity because it is a weak electrolyte Methanol, CH;OH, cannot conduct electricity but LIOH can. Acetic acid is a better conductor of electricity than chloric acid. I. II. III. IV.
Based on the solubility rules, which of the following should be soluble in water? Select one: а. Mу3(РО4)2 b. Sr3(PO4)2 c. Ag2S03 d. Na3PO4 е. BaSO4
True or False:
What is the mass of solute, in grams, in 300. ml. of a 1.299 x 10 M solution of NaPO,? Mass of solute- What are the molar concentrations of the Na and PO, ions? Molar concentration Na- Molar concentration PO, M