1. A patient has been admitted to the hospital with severe dehydration due to constant vomiting and diarrhea for the past 3 days. The first thing the hospital staff needs to do for this patient is administer fluids intravebously, but the patient is demanding he only be given "pure" water, and is refusing any other IV fluids. You are responsible for patient education at this hospital In order to get the patient to agree to be administered the 0.9% saline IV fluids he needs to rectify his dehydration, you must first educate him on what will happen if he exposes his cells to "pure" water. Explain to this patient why he should not receive pure water intravenously,

How do I solve this?

Consider a 0.37 M solution of CaCl2. What is the concentration of chloride ions in this solution in units of M?

I need help solving the following problem. How many grams of iodine potassium iodide would it take to obtain a 100 mL solution of 0.300 M IKI? Note: Recall that “IKI” is an abbreviation for iodine potassium iodide. The chemical formula is I3K and the molecular mass is 419.8 g/mole.

Describe how to prepare each of the following aqueous solutions, being specific about how you would do it (what type of glassware, size, etc.) – don’t just perform the calculations: a) 2.00 L of a 5.00 M aqueous solution of ammonium hydroxide from the concentrated solution (14.5 M). b) The solution shown to the right (0.9%) from solid sodium chloride and water. Remember, you want your patient to live!

Part C. Solubility versus Temperature 1. (a) Which solution(s) containing 1.0 g of salt (NaCl and NH,CI are both considered "salts") per 5 ml. of water is (are) unsaturated and why? 2. (a) Temperature of each solution before heating: NaCl: NH,Cl: (b) Which solution(s) containing 2.4 g total of salt per 5 ml of water is (are) saturated at room temperature and why? 3. (a) Temperature of each solution in the hot water bath: NaCl: NH.CI: (b) Which salt is least soluble at elevated temperatures? (c) Classify the salt solutions at elevated temperatures as either saturated or unsaturated. NaCl: NH.CI: 4. (a) Did the salt solution(s) that were unsaturated at the elevated temperatures become saturated when cooled? How do you know? 6.

. Suppose two beakers are placed in a small closed containerat 25°C. One contains 400 mL of a 0.100-M aqueous solution of NaCl; the second contains 200 mL of a 0.250-M aqueous solution of NaCl. Small amounts of water evaporate from both solutions. As time passes, the volume of solution in the second beaker gradually increases, and thatin the first gradually decreases. Why? If we wait longenough, what will the final volumes and concentrations be?

Stiller Paragraf 4) How many grams of sodium hydroxide does it take to make a 1 M 25 ml sodium hydroxide solution?

Select either True/False to state whether the following definition is correct for the following term/principle (i.e. if it is correct, select "True"): Common lon Effect: The solubility of a material is unchanged when at least one of its conjugates are also present in the solution. True False Question 4 (1 Select either True/False to state whether the following definition is correct for the following term/principle (i.e. if it is correct, select "True"): Trend observed for the osmotic pressure of a solution: The osmotic pressure of a solution defined as the pressure required to encourage ion flow across a semipermeable membrane. This is known as a colligative property. True False

A solution consisting of 1.1 M NaNO3 and 2.0 M Ca(NO3)2- concentration: 668 osmol/L