D) the absence of charged molecules inside cells. Answer: C Page Ref: Section 3 11) The ________ pressure is the pressure required to prevent the flow of solvent through a solvent-permeable membrane that separates two solutions of different solute concentration. A) hydrostatic B) electromotive Answer: C Page Ref: Section 3 12 C) osmotic D) partial 12) Which is true about the solubility of electrolytes in water? A) They are all insoluble in water. B) They are usually only sparingly soluble in water.
Name: ___________________________________ Date: ______________ Practice Test #3 ____ 1. When a precipitation reaction occurs, the ions that do not form the precipitate A) evaporate B) are cations only C) form a second insoluble compound in the solution D) are left dissolved in the solution E) none of these 2. An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. The complete ionic equation contains which of the following species (when balanced in standard form)? A) B) C) D) E) ____ 3.
The simple addition of water to FeSO4 will not lead to the formation of FeSO4•7H2O. Determination of the number of molecules of water in a hydrate. If you do not know how many molecules of water are in one molecule of hydrate and want to find this out, it can be done by measuring the masses of the hydrate and anhydrous compound formed after the heating. For example, let’s assume that we do not know how many water molecules are attached to BaCl2. Let’s call this number X.
[2] A saturated solution is one that holds as much dissolved solute as possible at a given temperature, therefore only a small amount of a slightly soluble ionic compound is needed to produce a saturated solution of that compound. [2] The solubility of a salt is the amount of the salt that
I believe we did our procedures accurately. The precipitate was Zinc hydroxide which is amphoteric in nature. Meaning it can react both with acid and base to form salt. We got a white precipitate of zinc hydroxide and it reacted to make salt with both the base sodium hydroxide and the acetic acid. Our result would have been clearer to observe if we centrifuged it long enough because we might have lost some of the precipitate while washing it since it was not centrifuged long enough.
The solution added reacted by turning the solution into a transparent liquid. This reaction is endothermic because the solution HC1 and Na2EDTA added decreased the reaction as the equilibriums both shifted to the left. When Na2SO4 was added the equilibrium should have shifted to the left. The solution reacted by creating more HSO4 even more when the 10 drops of the sodium sulfate solution was added as the color changed to a much lighter solution. When NaHSO4 was added the equilibrium should have shifted to the
This explanation can be demonstrated in table 3 also because the results of the reactions demonstrates that chloride reacted more by the color of the product compared to the color of chloride in the mineral oil. Also it also demonstrates that iodine is the weakest oxidizing agent because the results show that iodide didn’t change much from the color that it showed in the mineral oil. In example 6 we have shown the activity series for the halogens used in this
It was concluded that the most cost-effective bottle was the Tums Regular Strength due to it containing nearly the same amount of calcium carbonate listed on the bottle with a percent error of 4% while the other products contained higher percent errors. As well, the Tums Regular Strength tablet neutralized the second most amount of acid on
Introduction: You are aware that sugar dissolves in water but oil does not. What factors determine whether one substance will dissolve in another? A solvent is a substance that is capable of dissolving other substances and forming a homogeneous mixture called a solution. The substance dissolved is called the solute and is the component present in the smallest amount. The dissolving process involves a consideration of the relative strength of three intermolecular attractive forces.
(3) (b) An oil sample containing 0.0100 mol of oil was found to react with 7.61 g of iodine, I2. Determine the number of C=C double bonds present in each molecule of the oil. (b) [pic]= 0.03 (mol) 3 (double bonds) (ECF); 2 Correct answer scores [2]. If 6 is given, with no working, award [1]. (2) [May 2006 SL P3] ER: In (a), the structure of glycerol was well known by the better candidates, although quite a number of alcohols with only one –OH group, or with more than one –OH group on the same carbon, were seen.