Particulate Representations of lonic Solutions When AgNO, reacts with NaCl, a precipitate of AgCl(s) forms. The molecular equation for this reaction is: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) 1. Shown below is a particle diagram of a drop of 0.50 M NaCl. In the empty box, draw a particle diagram of a drop of 0.50 M AgNO,, assuming both drops have the same volume. Key + Na+ CI- Ag+ NO3- would be HAND

Particulate Representations of lonic Solutions When AgNO, reacts with NaCl, a precipitate of AgCl(s) forms. The molecular equation for this reaction is: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) 1. Shown below is a particle diagram of a drop of 0.50 M NaCl. In the empty box, draw a particle diagram of a drop of 0.50 M AgNO,, assuming both drops have the same volume. Key + Na+ CI- Ag+ NO3- would be HAND

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...

See similar textbooks

Similar questions

For the reaction Ba(OH)2 (aq) + (NH4)½CO3 (aq)--> What one of the following species would appear in the molecular equation? (Don't worry about coefficients. Just write the molecular equation, and see which of these appears in it.) OH (s) Ba2 (aq) O NH,OH (s) BaCO3 (s) O NH2"(aq)
The maximum contaminant level of cyanide (CN) in drinking water as set by the the Environmental Protection Agency (EPA) is 0.00020 g · L. Express this concentration in parts per million (ppm). Assume the density of water is 1.00 g/mL. concentration: Ppm
Consider the following chemical reaction. 3 Zn(C₂H₃O₂)₂(aq) + 2 Na₃PO₄(aq) → 6 NaC₂H₃O₂(aq) + Zn₃(PO₄)₂(s) A chemist makes a solution of zinc acetate by dissolving 20.5 g Zn(C₂H₃O₂)₂ in 105 mL H₂O. What is the concentration of this zinc acetate solution?
Insoluble PbBr2(s) precipitates when solutions of Pb(NO3)2 and NaBr are mixed. Pb(NO3)2(aq) + 2 NaBr(aq) ----------> PbBr2(s) + 2 NaNO3(aq) 200.0 mL of 0.750 M Pb(NO3)2 and 200.0 mL of 1.50 M NaBr are mixed together in a coffee cup calorimeter. The temperature of the mixture rises by 2.44°C. Calculate whether a limiting reactant is present or if perfect amounts of both reactants are present. Calculate the enthalpy change for this precipitation reaction. (assume the density of all solutions is 1.00 g/mL). (Answer in kJ)
If 785 mL of 0.350 M AgNO₃ is added to 475 mL of 0.250 M CaBr₂, how many moles of AgBr precipitate will be formed? The balanced equation is 2 AgNO₃(aq) + CaBr₂(aq) → 2 AgBr(s) + Ca(NO₃)₂(aq)
Potassium iodide reacts with lead(II)(II) nitrate in the following precipitation reaction: 2KI(aq)+Pb(NO3)2(aq)→2KNO3(aq)+PbI2(s)2KI(aq)+Pb(NO3)2(aq)→2KNO3(aq)+PbI2(s) What minimum volume of 0.218 MM potassium iodide solution is required to completely precipitate all of the lead in 145.0 mLmL of a 0.150 MM lead(II)(II) nitrate solution?
Find the volume of 0.339 M HCl(aq) required to completely neutralize 0.278 g of Al(OH)3(s) according to the unbalanced reaction: HCl(aq) + Al(OH)3(s) → AlCl3(aq) + H2O(l) The molar mass of Al(OH)3 is 78.0 g/mol. Give the answer in mL with 3 or more significant figures.
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…
While working in a lab, Ronan reacts 50.0 mL of 0.320 mol/L Na2CO3 (aq) with 85.0 mL of 0.210 mol/L AlCl3 (aq). Calculate the mass of Al2(CO3)3 precipitate that forms when the reaction is complete 3 Na2CO3 (aq) + 2 AlCl3 (aq) → Al2(CO3)3 (↓) + 6 NaCl (aq)
4. Calculate the calculate the mass of precipitate formed from 5.0 g of strontium chloride. Li3PO4(aq) → Sr3(PO4)2(S) + LiCl(aq) _SrCl₂(aq) + 5. What mass of aluminum hydroxide in needed to neutralize 5.00 g of hydrochloric acid? Al(OH)3(s) + _HCl(aq) → ___AlCl3(aq) + _H₂O(1) 195
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)
The metathesis reaction between iron (III) nitrate and sodium hydroxide is shown belowFe(NO3)3 (aq) + 3 NaOH (aq) ➝ 3 NaNO3 (aq) + Fe(OH)3 (s)How many grams of solid iron (III) hydroxide can be produced by the reaction of 50.0 ml of 0.650 M iron (III) nitrate solution with 150.0 ml of 0.750 M sodium hydroxide solution?The formula weight of Fe(OH)3 = 106.866 g/mol.Answer grams of Fe(OH)3.Determine the final concentration of each ion in solution at the end of the precipitation reaction. NO3− Answer M Fe+3 Answer M OH− Answer M