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4) nickel (II) chloride and lead (II) nitrate 5) chromium (II) bromide with lithium oxalate -...
Net lonic Equations: For each of the following reactions, you will need to write (a) the molecular equation, (b) the ionic equation, and (c) the net ionic equation. You will need to interpret the chemical names into (neutral chemical) formulas and complete the reactions. Be sure to write balanced chemical reactions as well as provide the correct state of matter for each compound in all of your reactions (solubility rules.) Please attach images of your work to receive credit. 5)...
SUPPLEMENTAL EXPERIMENT - NET IONIC EQUATIONS Name: AM PM LAB For each of the following reactions, you will need to write (a) the molecular equation, (b) the ionic equation, and (c) the net ionic equation. You will need to interpret the chemical names into (neutral) chemical formulas and complete the reactions. Be sure to write balanced chemical reactions as well as provide the correct state of matter for each compound in all of your reactions (solubility rules) 1) potassium phosphate...
SUPPLEMENTAL EXPERIMENT - NET IONIC EQUATIONS Name: LAB AM PM For each of the following reactions, you will need to write (a) the molecular equation, (b) the ionic equation, and (c) the net ionic equation. You will need to interpret the chemical names into (neutral) chemical formulas and complete the reactions. Be sure to write balanced chemical reactions as well as provide the correct state of matter for each compound in all of your reactions (solubility rules) → 11) acetic...
Reaction 14: Aqueous iron(II) chloride + aqueous ammonium hydroxide Balanced Molecular Equation (from page 8): Complete lonic Equation: Net Ionic Equation: 2. Predict the products for the followine single and double displacement reactions, and wing single and double displacement reactions, and write balanced molecular squations including physical states) for each of them. If you predict that no reaction will occur, w na reaction will occur, write "NR", " followed by a brief explanation. a. Aluminum metal + aqueous silver acetate...
Study Exercise 3 Name Write chemical formulas for the following compounds: 1. 2. 3. Potassium iodide Barium sulfate Aluminum nitrate Copper (II) carbonate Gold (III) chloride Ferric hydroxide 7. Lead (II) chromate Nickel (II) hydroxide Mercury (II) bromide Silver acetate Magnesium chlorate 12. Sodium peroxide 13. Manganese (II) phosphate Ammonium sulfide 15. Platinum (IV) fluoride Chromium (III) hydroxide Calcium oxalate Antimony trichloride Ammonia Silicon dioxide Carbon monoxide 22. Hydrobromic acid Nitrous acid 24. - Acetic acid 25. Sulfuric acid
A. silver nitrate, AgNO3, and magnesium bromide, MgBr2 net ionic equation: _______ B. perchloric acid, HCIO4, and potassium hydroxide, KOH net ionic equation: _______ C. ammonium sulfide, (NH4)2S, and cobalt(II) chloride, CocI2, net ionic equation: _______
Question 18 (3 points) Which of the following is a (are) common moderate base(s)? transition metal hydroxides, Group IIIB (3) scandium thru IIB (12) zinc aqueous ammonia and aqueous magnesium hydroxide u nqueous ammonium hydroxide aqueous ammonia as aqueous ammonium hydroxide and aqueous lithium hydroxide Question 19 (3 points) Which of the following isare) common strong acids? hydroiodic acid, hydrobromic acid, hydrochloric acid and hydrofluoric acid perchloric acid, chloric acid and hydrochloric acid nitric acid, sulfuric acid, phosphoric acid, and...
help! Section 1: Balance each of the following reactions. Your instructor may discuss the different types of reactions present in these examples. Reaction Type Al + O2 +Al:03 Synthesis Synthesis N2 + H2 + NH3 MgCO3 → MgO + CO2 KCIO: → KCI + 02 Cu + AgNO3 → Ag + Cu(NO3)2 Cl2 + Nal → NaCl + 1; HCI + NaOH + H:0 + NaCI BiCl3 + H2S → Bi2S3 + HCI Section II: Balance each of the following...
Page 157 IONIC AND NET IONIC EQUATIONS Some Solubility Rules: (a) Group 1A, ammonium, acetate, and nitrate compounds are soluble. (b) Chloride, bromide, and iodide compounds are soluble except silver, lead(II) and mercury(1). (c) Carbonates and phosphates are insoluble except for Group IA and ammonium compounds. (d) Hydroxides are usually insoluble except for Group IA, strontium, barium and ammonium compounds. (e) Sulfides are usually insoluble. Some exceptions are Group IA and ammonium compounds Use the solubility rules given above and...
Lab 8: Identification of Metallons and Inorganic Compounds by their Chemical Reactions Kotification of Metalowes and organic Compounds by their Chemical Reactions 3. Write balanced formula unit and net ionic equations for each of the following chemical reactions in aqueous solution. If no reaction occurs, write NR. Include the states (s, lg, or aq) of all reactants and products. A. copper(II) chloride + lead(II) nitrate B. zinc bromide + silver nitrate - C. iron(III) nitrate + ammonia solution - D....