Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- 60 Types of Chemical Reactions 6) Get two medium test tubes. Into one, place about 2 mL of a solution of hydrochloric acid. Into the other add about 2 mL of a solution of sodium hydroxide. Note the appearances of the contents in the two test tubes and then mix them together noting any changes that have taken place. Change(s) that took place when the solutions were mixed: Balanced Chemical equation: Balanced ionic equation: Balanced net ionic equation: H+ + OH - → H₂0 (1) 7) Get two medium test tubes. Into one, place about 2 mL of a solution of copper(II) sulfate. Into the other add about 2 mL of a solution of sodium phosphate. Note the appearances of the contents in the two test tubes and then mix them together noting any changes that have taken place. Change(s) that took place when the solutions were mixed: Balanced Chemical equation: Balanced ionic equation: Balanced net ionic equation: Gefarrow_forwardIdentify each of the following as precipitation, acid/base, oxidation/reduction, or combustion. A) Mg(OH)2(6) + 2 HClaq) → 2 H,O@ + MgCl(aq) B) Na,SO4(aq) + Ca(NO3)2(aq) → 2NaNO3(aq) + CaSO4(6) C) Zncs) + Cu(NO3)2(ag) → Zn(NO3)2(aq) Cue) +arrow_forwardWill precipitation occur when the following solutions are mixed? ▾ Part D ▼ Write a balanced chemical equation for the reaction. Li2CO3 and AgNO3 Express your answer as a chemical equation including phases. ΑΣΦΑ A chemical reaction does not occur for this question. Submit Request Answer Part E ? Write a balanced chemical equation for the reaction. ZnSO4 and Pb(NO3)2 Express your answer as a chemical equation including phases. ΑΣΦ ?arrow_forward
- You have three soultions: Na2CO3, BaCl2 and KNO3. You also have four reagents, HCl, CaCl2, NaOH, and H2SO4, that can help you identify all three solutions. Which one of these reagents can you use to be able to identify and label all three solutions? Explain your reasoning. Include any net ionic equations for precipitation reacions.arrow_forwardWrite the net ionic equation for the following molecular equation. HCl is a strong electrolyte. HF is a weak electrolyte. NaF(aq) + HCl(aq) → NaCl(aq) + HF(aq) (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank.)arrow_forwardSo I have figured out the right balanced equation in the first picture but I cannot figure out the net ion equation. I know that I do not include the spectator ions in a net ionic equation and to me the spectator ions would be the hydroxide ions (if Al(OH)3 dissociated in water) and the H+ ions but since aluminum hydroxide does not dissociate then it must be included in the net ion equation as Al(OH)3 so I would think that the net ion equation would be Al(OH)3(s) + 3Cl-(aq) -> AlCl3(aq) but that was the first thing I tried and it was wrong, so I tried adding in the 3H2O that gets made but that was wrong, so I added in the H+ ions and that still wasn't right, I cannot see where I am going wrong here. Please help!arrow_forward
- What is(are) the spectator ion(s) for the following reaction?Ag2NO2 + HI → No spectator ion. All ions are spectator ions, no reaction. NO2‾ H+ and NO2‾arrow_forwardUse the precipitation interactive to answer the questions. Select the color of the solid that forms when Ni(NO3)2Ni(NO3)2 solution is added to K2SK2S solution. white green black yellow Complete the net ionic equation for the reaction. Cation ++ Anion ⟶⟶ Precipitatearrow_forwardYou have aqueous solutions of Ag* and PO43- that have equal concentrations. You mix them according to the following table: Test Tube # Number of drops Ag Number of drops PO4³- 01 0 4 2 1 3 3 9 2 t 8 3 6 4 Assuming the product of the reaction is insoluble, which test tube will contain the most. precipitate? 8 5 9 3arrow_forward
- -N 1 Osynthesis Oprecipitation c. Classify the reaction represented by the following unbalanced equation by as many methods as possible. Choose the correct balanced equation. FeCl₂ (aq) + AgNO3(aq) → Fe(NO3)2 (aq) + AgCl(s) (Select all that apply.) oxidation-reduction decomposition [Review Topics] Osingle-displacement Odouble-displacement FeCl₂ (aq) + 2AgNO3(aq) → Fe(NO3)2 (aq) + 2AgCl(s) FeCl₂ (aq) + 2AgNO3(aq) → Fe(NO3)2 (aq) + AgCl(s) (Select all that apply.) Doxidation-reduction Odecomposition Osynthesis Oprecipitation Osingle-displacement Odouble-displacement d. Classify the reaction represented by the following unbalanced equation by as many methods as possible. Choose the correct balanced equation. Al(s) + Br₂ (1)→→ AlBr3 (8) [References] 2Al(s) + 3Br2 (1)→ 2A1Br3 (8) Al(s) + 3Br2(1)→ AlBr3 (s)arrow_forwardHelp pleasearrow_forwardDetermine net ionic equations, if any, occuring when aqueous solutions of the following reactants are mixed. Select "True" or "False" to indicate whether or not the stated reaction (or "no reaction") correctly corresponds to the expected observation in each case. Magnesium chloride and sodium hydroxide; No reaction occurs. Sodium bromide and hydrochloric acid; No reaction occurs. Copper(II) sulfate and ammonium carbonate; No reaction occurs. Nickel(II) chloride and lead(II) nitrate; No reaction occurs. Sodium phosphate and potassium nitrate; 2Na+ (aq) + NO2- 3 (aq) ------> Na2NO3(s)arrow_forward
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