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 laboratory, you are given the task of separating Ba2+ and Co2+ ions in an aqueous solution. For each reagent listed below, indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" Y or N Reagent Formula of Precipitate if YES HCl Na2S K2CO3
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.
Write the balanced precipitation reactions
Use the solubility rules from your textbook to answer the following questions regarding mixtures of unknowns. If one of your test tubes contained both Ca2+andAg+, would you be able to somehow separate them by adding NaCl(aq)? Use equations to explain your answer. What if the solution contained Na+and K+? Would the addition of NaOH help you separate them?
You have an unknown solution and you want to determine if it contains ammonia. How will you detect its presence in the laboratory analysis? Please provide two ways to analyze its presence and explain your chosen technique in determining the ammonia.
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
Write the equation for the dissolving of iron(II) hydroxide in water. Be sure to specify the state of each reactant and product. +
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…
A student determined the concentration of copper by ion exchange. He obtained the following results: 28.61 mL of 0.0810 M NaOH solution was required to titrate the eluate (HCl solution) from the column. He used 15.0 mL sample of copper chloride solution initially. Calculate the number of moles of H+ present in the eluate.
Predicting precipitation 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 empirical formula of precipitate form solution A solution B when A and B precipitate are mixed? ? manganese(II) chloride zinc sulfate yes no ammonium bromide sodium acetate yes no iron(II) sulfate sodium sulfide yes no