A pair of students are completing an experiment in lab. They mix aqueous sodiumchloride with aqueous calcium nitrate. The solution looked clear in their test tube. Thelab manual states, "All common nitrates (NO3) are soluble. All chloride (CI) ions aresoluble except with Ag*, Cu*, and Pb2+."%3DSelect the chemical reaction that shows the correct, balanced chemical reactionbetween sodium chloride and calcium nitrate.2 NaCI (aq) + Ca(NO3)2 (aq) → CaCl2 (aq) + 2 NANO3 (aq)2 NaCI (aq) + Ca(NO3)2 (aq) → CaCl2 (s) + 2 NaNO3 (aq)NaCI (aq) + Ca(NO3)2 (aq) → no reaction2 NaCI (aq) + Ca(NO3)2 (aq) → CaCl2 (aq) + 2 NANO3 (s)

Here we are mixing aqueous sodium chloride (NaCl) with aqueous calcium nitrate Ca(NO3)2 So, sodium…

A pair of students are completing an experiment in lab. They mix aqueous sodium chloride with aqueous calcium nitrate. The solution looked clear in their test tube. The lab manual states, "All common nitrates (NO3) are soluble. All chloride (CI') ions are soluble except with Ag*, Cu*, and Pb2*." Select the chemical reaction that shows the correct, balanced chemical reaction between sodium chloride and calcium nitrate.

A pair of students are completing an experiment in lab. They mix aqueous sodium chloride with aqueous calcium nitrate. The solution looked clear in their test tube. The lab manual states, "All common nitrates (NO3) are soluble. All chloride (CI') ions are soluble except with Ag, Cu, and Pb2*." Select the chemical reaction that shows the correct, balanced chemical reaction between sodium chloride and calcium nitrate.

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

Two solutions are mixed, and the resulting reaction produces NaNO3(aq) and NiCO3(s). a. Write the balanced molecular equation for this reaction. b. Write the net ionic equation, given that the sodium and nitrate ions are the spectator ions.
A sample is a mixture of the salts and silver nitrate, copper (II) chloride, and iron (III) chloride. When a 1.000 g sample of the mixture is dissolved in water and reacted with excess silver nitrate, 1.7809 g of precipitate forms. When a separate 1.000g sample of the mixture is treated with a reducing agent, all the metal ions in the sample are reduced to pure metals. The total mass of the metals produced is 0.4684g. Calculate the percent of each salt in the original mixture.
0.8888 g a mixture contains calcium chloride and potassium nitrate. To determine the % of each compound, silver nitrate was added to these solutions to precipitate all the chlorine in a form of silver chloride. 1.885 grams of silver chloride was precipitated, washed and dried. Calculate the % of calcium chloride in the sample.
8. A student adds 22.36 mL of 1.366 x 10¹ M Mg(OH), in order to completely neutralize 25.00 mL of H₂PO acid. Calculate the original concentration of the acid solution.
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, provide the net ionic equation. KI+ Pb(NO3)2
A pair of students are completing an experiment in lab. They mix solid sodium carbonate with aqueous hydrochloric acid. The solution produces bubbles in their test tube. The lab manual states, "All common nitrates (NO3) are soluble. All carbonates (CO3)2- are insoluble except with group 1 or NH4* ions. All chloride (Cl') ions are soluble except with Ag*, Cu*, and Pb2+." Select the chemical reaction that shows the correct, balanced chemical reaction between sodium carbonate and hydrochloric acid. Na2CO3 (s) + 2 HCI (aq) → 2 NaCI (aq) + H2CO3 (s) Na2CO3 (s) + HCI (aq) → No reaction Na2CO3 (s) + HCI (aq) → NaCI (aq) + CO2 (g) + H20 (1) Na2CO3 (s) + 2 HCI (aq) → 2 NaCI (aq) + CO2 (g) + H2O (1)
In an experiment, a student combines 75.0 mL of a 0.190 M iron (III) chloride solution with 125.0 mL of a 0.240 M sodium carbonate solution. a. Write a balanced equation for the reaction to see how many grams of sodium chloride need to be produced in the experiment in order to achieve a yield of 83.75%?
Cobalt(II) chloride solution reacts with sodium hydroxide solution. Identity the spectator ion(s). Note: you may choose more than one answer. O Co2+ Na OH
Write the net ionic equation.
1. Aqueous copper (II) sulfate and 0.75 M sodium hydroxide react to form a precipitate of copper (II) hydroxide and aqueous sodium sulfate. Write the chemical equation for this reaction. Classify this reaction and write the general form for this type of reaction equation If both solutions were clear add the beginning of the reaction, why does this reaction form a blue solid precipitate? 2. Solid zinc metal reacts with aqueous hydrogen monochloride to form aqueous zinc chloride and hydrogen gas. Write the symbolic form of this chemical reaction. Classify this chemical reaction and write the general form of this type of reaction. What could we do to verify that the gas released was, in fact, hydrogen? Is zinc chloride soluble or insoluble in water? How do you know?
A 20.91 mL solution containing 1.678 g Mg(NO3), is mixed with a 26.79 mL solution containing 1.215 g NaOH. Calculate the concentrations of the ions remaining in solution after the reaction is complete. Assume volumes are additive. If a species fully precipitates, type 0. Be sure your answer has the correct number of significant digits. M Mg 2+ ΜΝΟ, M Na M OH x10 X S