a student mixes sodium chloride and water until the solid and the aqueous solution are at...
In a lab. silver nitrate, AgNO_3, is dissolved in water until no solid is observed in the container Then a solution of sodium chloride. NaCl. is added to the container When you combine these aqueous solutions, there is no noticeable change in temperature, however, a solid properties and there is a slight change of color. Which statements about the lab experiment involving silver nitrate and a sodium chloride solution are true?
Imagine the following scenario: a student doing the experiment added 20 mL of silver nitrate, AgNO3, to the blue equilibrium mixture. The reaction mixture become pink and cloudy with white precipitate of silver chloride , AgCl, appearing in the bottom of the flask. Can you explain how those observations are consistent with Le Chatelier's principle? Imagine the scenario: A student placed pink equilibrium mixture in the hot water. Reaction mixture changed color to blue. Is the reaction endothermic or exothermic?...
Name Part B. Iron un Chloride (FeCl) plus Potassium Thiocyanate (KSCN Prepare a stock solution to be tested by adding 12 drops each of 0.1 M FeCl, and 0.1 MKSON well. Fill each of four medium sized test tubes (all the same size) half full of the stock solution FeSCN'(a) pale yellow colorless 1. The first tube is a control. Always compare to this color. 2. Add 20 drops of 0.1 Miron () chloride solution to the second tube. Observe...
2. (4 points) A chemist must dilute 34.7 mL of 2.77M aqueous sodium chloride solution until the concentration falls to 2.00 M . He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters.
A chemist must dilute 59.9 mL of 1.59 M aqueous sodium chloride (NaC1) solution until the concentration falls to 1.00 M. He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters. Round your answer to 3 significant digits.
compare the solid sodium chloride conductivity to aqueous sodium chloride solution conductivity. How come the values are different?
#8 10. Rewrite the nee d ed Part II. Dissolution of malum chloride a water Section A 1. Initial appearance of equilibrium m e Clear 2. Change after addition of cone HICH cloudy Nhile 3. Change after heating mature for 3-4 min Clear 4. Change after cooling mixture Section B Cloudy White Observations of dissolution of solid NH.C in water, The dissolution is cold, Conclusions 5. The equation for the dissolution of NHCl in water is: NH.C($) 5 NH' (aq)...
Experience teaches us that most solids are more soluble in warm water than in cold water. Does the solid utility of Mg(OH)_2 fit this pattern? Briefly explain. Cobalt chloride is used in many weather-forecasting devices. Based on your observations in the laboratory, explain how an alcohol solution of CoCl_2 could be used to predict rain. A student is studying the equilibrium described by the net ionic equation shown in Equation 18. [Cu(H_2O)_6]^2+ (aq, blue) + 4 Br^-(aq) CuBr_4^2+(aq, green) +...
At room temperature, you are given a litre of a solution of PbCl2(aq)inwhich there is excess PbCl2(s)i.e. a saturated solution. State and explain the effect of the following on the concentration of the Pb2+ ions in the solution? [Remember to use ideas on equilibrium, Le Chatelier's Principle, etc. in your answer] Adding more PbCl2 solid Adding NaClsolid Adding 500 ml of water, assuming there will still be excess solid afterwards. Heating the solution to 35 0C assuming the solubility is...
Aqueous hydrochloric acid will react with solid sodium hydroxide to produce aqueous sodium chloride and liquid water . Suppose 24.8 g of hydrochloric acid is mixed with 16. g of sodium hydroxide. Calculate the maximum mass of sodium chloride that could be produced by the chemical reaction. Be sure your answer has the correct number of significant digits