Question 21 You have plenty of salts that are in front of you and you are trying to figure out which salts are soluble in water, and which ones of their products are soluble in water. For the following equation, identify which reactants and products are soluble/insoluble in water. H₂SO4+ Ba(OH)₂ -> Use the editor to format your answer Question 22 You have plenty of salts that are in front of you and you are trying to figure out which salts are soluble in water, and which ones of their products are soluble in water. For the following equation, identify which reactants and products are soluble/insoluble in water. Kl+ Pb(NO3)2 ->

Question 21 You have plenty of salts that are in front of you and you are trying to figure out which salts are soluble in water, and which ones of their products are soluble in water. For the following equation, identify which reactants and products are soluble/insoluble in water. H₂SO4+ Ba(OH)₂ -> Use the editor to format your answer Question 22 You have plenty of salts that are in front of you and you are trying to figure out which salts are soluble in water, and which ones of their products are soluble in water. For the following equation, identify which reactants and products are soluble/insoluble in water. Kl+ Pb(NO3)2 ->

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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- Part C Write a balanced ionic equation for this acid-base reaction: Ca(OH)2 (aq) + 2CH3CO₂H(aq) → Express your answer as a chemical equation. Identify all of the phases in your answer. ΑΣΦ A chemical reaction does not occur for this question. Submit Request Answer Part D ? Write net ionic equation for this acid-base reaction: Ca(OH)2 (aq) + 2CH3CO₂H(aq) → Express your answer as a chemical equation. Identify all of the phases in your answer.
"In the lab, a student makes a solution of NaOH by dissolving 49.0 grams of solid in 195 mL of water. What is the molarity of the NaOH solution that the student prepared? The molar mass of NaOH is 39.9971 g/mol." 6.28 M 7.28 M 0.00628 M 0.419 M 10.1 M
10. The equations below represent precipitation reactions. Rewrite these as complete ionic and net ionic equations. Molecular Equation Complete Ionic Equation Net Ionic Equation Molecular Equation Complete lonic Equation Net Ionic Equation AgNO, (aq) + KCI (og) → KNO, (aq) + AgCl (s) Molecular Equation Complete Ionic Equation Net Ionic Equation Ba(ClO4)2 (aq) + K₂SO4 (ng) BaSO (s) + 2 KCIO₂(g) 11. The equation below represents a neutralization reaction. Rewrite this as complete ionic equations and net ionic equations. 2 HCl(aq) + Ba(OH)2 (aq) → 2 H₂O )+ BaCl₂ (aq) Include phase symbols.
6. Sodium sulfide reacts with hydrochloric acid to produce hydrogen sulfide and sodium chloride. How many grams of sodium sulfide are required for complete reaction with 15.0 mL of 0.250 M hydrochloric acid? The molar mass of sodium sulfide is 78.046 g/mol. (Hint: start by writing the balanced equation for the reaction.)
Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. Does a precipitate form when A and B are empirical formula of solution A solution B precipitate mixed? iron(II) iodide zinc sulfate O yes O no sodium sulfide iron(II) chloride yes no potassium hydroxide zinc nitrate О yes no
Equation 1: X(s) + NiCl2 (aq) Equation 2: X(s) + MgCl, (aq) → no reaction Ni(s) + XCl, (aq) A sample of an unknown solid metal, X(s), is added to a solution of NiCl, (ag), which results in the formation of Ni(s) and XCl, (ag). When a sample of X(s) is added to a solution of MgCl2 (aq), no changes are observed. The results of the experiment are summarized in equations 1 and 2. Which of the following represents a possible identity of metal X and provides the correct justification? A Cu, because Cu is oxidized more easily than both Mg and Ni. Cu, because Cu is oxidized more easily than Ni but less easily than Mg. Zn, because Zn is oxidized more easily than both Mg and Ni. Zn, because Zn is oxidized more easily than Ni but less easily than Mg. Sign out acer 06
Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. Does a precipitate form when A and B empirical formula of solution A solution B precipitate are mixed? ammonium sulfide copper(II) nitrate O yes O no potassium chloride ammonium nitrate O yes O no iron(II) iodide zinc sulfate O yes O no
Write the balanced formula equation for this reaction: HCl + NH3 → Enter your answer as the sum of coefficients. Determine the balanced total ionic equation for the same reaction and enter the sum of the coefficients.
You titrate a 25.00 mL solution of hydrochloric acid, HCI, with a 0.2015 M sodium hydroxide, NaOH, solution. The titration required 39.73 mL of the sodium hydroxide to reach the endpoint. What is the concentration (molarity) of the hydrochloric acid? HCI + NaOH → NaCl + H₂O Student work: 39.73 mL NaOH 1 L 1000 ML 25.00 mL HCI 1000 mL HCI 1 L HCI 0.0080055 mol HCI 0.02500 L HCI 0.2015 mol NaOH 1 L NaOH 0.02500 mol 0.3202 M HCl 0.0080055 mol Read the feedback statements below and chose all that are applicable to the work shown. Choose one or more: The unit cancellation is not correct. The conversions to from mL to L do not need to be shown since they cancel out. O The final answer has an incorrect number of s.f. (it should have 4 s.f.) U The final answer has an incorrect number of s.f. (it should have 3 s.f.) [] Units do not cancel properly. The stoichiometry step to convert mol NaOH to mol HCI is not shown. U All data collected, work shown, and final answer are recorded and shown…
Suppose a student performs a similar reaction using sodium bicarbonate (NaHCO3) instead of sodium carbonate. The sodium bicarbonate is dissolved in water, and a solution of 6.0 M HCl is added to the sodium bicarbonate in increments. Bubbles are observed during the reaction. The data collected is shown in the table. moles of NaHCO3: mass of empty beaker (g) moles of NaCl: mass of beaker and NaHCO3 (g) initial volume of 6.0 M HCl (mL) How many moles of NaHCO3 were used? balanced equation: final volume of 6.0 M (ml) mass of beaker and NaCl (g) How many moles of NaCl were produced by the reaction? Write the balanced chemical equation for the reaction. Include physical states. 84.000 g 86.279 g 20.0 mL 12.0 mL 85.585 g mol mol
Add all four reaction steps together to get the overall reaction. Remember to cross out anything that occurs on both the reactant and product sides and to combine like terms. 1. 2 Al(s) + 2 KOH (aq) + 6 H2O (l) → 2 KAl(OH)4(aq) + 3 H2(g) 2. 2 KAl(OH)4(aq) + H2SO4 (aq) → 2 Al(OH)3(s) + 2 H2O (l) + K2SO4(aq) 3. 2 Al(OH)3(s) + 3 H2SO4 (aq) → Al2(SO4)3(aq) + 6 H2O (l) 4. Al2(SO4)3(aq) + K2SO4(aq) + 24 H2O (l) →2 (KAl(SO4)2∙12H2O) (s) For each reactant except water, calculate the number of moles you added (use the stoichiometry of the balanced equation to identify the limiting reactant. Al: ____ moles KOH: ____ moles H2SO4: ____ moles mass of aluminum: 0.49g the volume of 1.4 M KOH: 25.0 mL the volume of 9 M H2SO4: 10.2 mL mass of watch glass: 50.28 g mass of watch glass plus alum: 58.17g
Listen Which equation below correctly describes the formation of a solution of calcium chloride in water? A) CaCl2(s) + H₂O (1)→ Ca2+ (aq) + Cl₂ (aq) B) CaCl2(s) + H₂0 (1)→ Ca²+(aq) +2Cl¯(aq) OC) OD) CaCl2(s) + H₂O (1) CaCl₂(aq) CaCl2(s) + H₂O (1)→ CaCl2(s)