Prepare 50 mL of an aqueous solution of 2.5% (w/v) NaCl (sodium  chloride, salt).Determine how many grams of sodium chloride are required. Show all steps for  this calculation, using dimensional analysis with units clearly identified. 2. Prepare this aqueous solution, using a volumetric flask for the precise final  volume measurement. It is not a problem to use tap water. 3. Clearly write the procedure (step by step) for making this solution

Why does the molarity of NaOH usually have to be standardized? When preparing the aqueous NaOH, the exact volume of the NaOH used cannot be measured due to water being hygroscopic. Solid NaOH can react with acid very easily and therefore the initial mass of the base may not be exact. When dissolving the solid NaOH in pure distilled water, the exact volume of the NaOH used cannot be measured due to buret calibration. Solid NaOH can react with water in the air very easily and therefore the initial mass of the base may not be exact.

b. the la. (1) Explain what is meant by the terms soluble, solute, solvent, and solution, illustrating your answer by reference to potassium chloride and water (!) Give an example of a substance which is insoluble in water Explain what is meant by the terms miscible and immiscible and give an example of two miscible liquids and two immiscible liquids. List and explain three general factors that affect the solubility of a gas in water [AC 2.1] 2. Explain with diagram, the structure and formation of the hydrated potassium ion and the Khydrated chloride ion. [AC 2.2] 3. (a) An acidic, aqueous solution of hydrochloric acid, HC1 (aq), has a pH of 2.5 (a) State which ions are present in the aqueous solution of hydrochloric acid. (b) Write balanced chemical equations to show the reactions which would occur solution of hydrochlóric acid was mixed with: mágnesium metal solid magnesium oxide (I) solid sodium carbonate, Na2CO3. (iii) Using answer to (a), explain why these reactions occur. to Hig

A glucose solution is 30.0% C6H1206 by mass. It is simultaneously 1.87 M at 20 °C. (a) Compute the density of this solution. Density = 8 cm-3 (b) What volume of this solution should be used in preparing 1.38 L of a 0.180 M glucose solution? Volume = mL

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.

The solute is the chemical that gets dissolved and it should be set to “Drink mix”. Adjust the volume to 1.0L and the solute amount to 1.0 mile . What is the molar concentration (“Molarity”)?

Ignore my calculations that are already on there, but I'm struggling on this one and a step by step would really help me out. Thank you!

Match the following aqueous solutions with the appropriate letter from the column on the right. Assume complete dissociation of electrolytes. 1.8.8E-2 m Fe(NO3)3 2. 0.14 m Na₂S CuSO4 Ethylene glycol (nonelectrolyte) 3. 0.19 m 4. 0.32 m ---- ---- ---- ---- A. Highest boiling point B. Second highest boiling point C. Third highest boiling point D. Lowest boiling point

7. During week l's lab we investigated the effect of different soaking solutions on the behavior of red blood cells. If the blood had arrived on time, our prepper would have needed to know how to make up different concentrations of saline (NaCl) solution from a 2.7% stock solution of NaCl. Can you help her by filling in the table below? For each group of students, you want to make 9ml of either 0.9% saline or 0.45% saline. Show your working out below the table you complete. 0.9 0.45 % saline solution wt/vol Volume of 2.7 2.7%wt/vol NaCl in ml Volume of distilled water in ml

How do I calculate the mass of Na2CO3 needed for the .25 ml of solution? Use the following image to help