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

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