When calcium nitrate reacts with ammonium phosphate, what precipitate will form? Wattemolecular equation, the complete ionic equation, and the net ionic equation.Potassium metal reacts hydrochloric acid to produce hydrogen gas and potassium chloride. If 3.0 moles ofpotassium reacts to form 2.0 moles of potassium chloride, how many moles of hydrogen gas are produced?The density of an ideal gas is 0.850 g/L at 25.°C and 380. torr. Calculate the molar mass of the gas.

Step 1:Firstly a balanced chemical equation is written. Step 2: Then using the stoichiometry,…

Answered: When calcium nitrate reacts with…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 114AP

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Calcium carbonate, CaCO3, can be obtained in a very pure state. Standard solutions of calcium ion are usually prepared by dissolving calcium carbonate in acid. What mass of CaCO3 should be taken to prepare 500. mL of 0.0200 M calcium ion solution?
Polychlorinated biphenyls (PCBs) have been used extensively as dielectric materials in electrical transformers. Because PCBs have been shown to be potentially harmful, analysis for their presence in the environment has become very important. PCBs are manufactured according to the following generic reaction: C12H10+nCl2C12H10nCln.+nHCl This reaction results in a mixture of PCB products. The mixture is analyzed by decomposing the PCBs and then precipitating the resulting Cl asAgCl. a. Develop a general equation that relates the average value of n to the mass of a given mixture of PCBs and the mass of AgCl produced. b. A 0.1947-g sample of a commercial PCB yielded 0.4791 g of AgCl. What is the average value of n for this sample?
What is the difference between a solute and a solvent?
ssume a highly magnified view of a solution of HCI that allows you to “see” the HCl. Draw this magnified view. If you dropped in a piece of magnesium, the magnesium would disappear, and hydrogen gas would he released. Represent this change using symbols for the elements, and write the balanced equation.
Nitric acid is produced commercially by the Ostwald process, represented by the following equations: 4NH3(g)+5O24NO(g)+6H2O(g)2NO(g)+O2(g)2NO2(g)3NO2(g)+H2O(l)2HNO3(aq)+NO(g) What mass of NH3 must be used to produce 1.0 106 kg HNO3 by the Ostwald process? Assume 100% yield in each reaction, and assume that the NO produced in the third step is not recycled.
You need to make a 0.300-M solution of NiSO4(aq). Calculate the mass of NiSO4 · 6H2O you should put into a 0.500-L volumetric flask.
Write the net ionic equation for the reaction, if any, that occurs on mixing (a) solutions of sodium hydroxide and magnesium chloride. (b) solutions of sodium nitrate and magnesium bromide. (c) magnesium metal and a solution of hydrochloric acid to produce magnesium chloride and hydrogen. Magnesium metal reacting with HCl.
4.49 Small quantities of hydrogen gas can be prepared by the following reaction: Zn(s)+H2SO4(aq)ZnSO4(aq)+H2(g) How many grams of H2 can be prepared from 25.0 mL of 6.00 M H2SO4 and excess zinc?
Describe in words how you would prepare pure crystalline AgCl and NaNO3 from solid AgNO3 and solid NaCl.
The flasks below illustrated three trials of a reaction between varying amounts of zinc and a constant volume of hydrochloric acid solution of constant concentration. The table gives the initial amount of zinc added and the observation at the conclusion of each reaction. Mass of Zinc Added g Observation at Conclusion of Reaction 6.10 Balloon inflated completely Some unreacted zinc remains 2.37 Balloon inflated completely No zinc remains 0.41 Balloon not inflated completely No zinc remains The reaction produces an aqueous solution of zinc chloride and hydrogen gas. Explain the observed results.
Write a chemical equation representing the decomposition of water into two gaseous products. What are the products?
What is the molarity of a solution of sodium hydrogen sulfate that is prepared by dissolving 9.21 g NaHSO4 in enough water to form 2.00-L solution? What is the molarity of each ion in the solution?

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