Sometimes as a solute dissolves in a solvent, the solute molecules dissociate and sometimes they associate. Explain how dissociation affects the molar mass of the unknown solute using this method.
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- 2. A student makes a standard solution of potassium hydroxide by adding 14.555g to 500.0mL of water. Answer the following questions, being sure to include units and remember sig figs. Show work. a. What is the concentration of this standard solution? b. If the student pours out a 15.6mL sample of this solution, how many moles of sodium hydroxide does the student have in the sample? 3. What possible issues many results from air bubbles in the burette for this experiment? Be specific about how this may affect the final calculated concentration of acid (Will it be lower or higher than actual? Why?)Table 1: Temp vs. solubility data of ammonium chloride. Test tube g NH4Cl/10 mL H2O Crystallization temp. (ºC) 1 1.0 g/10 mL H2O 10 oC 2 1.8 g/10 mL H2O 20 oC 3 2.9 g/10 mL H2O 40 oC 4 3.8 g/10 mL H2O 65 oC 5 4.4 g/10 mL H2O 95 oC Use the table to plot a solubility curve for ammonium chloride on the graph provided below. For the best fit line, use a smooth curve. "Mass of Solute per 100 mL of H2O," should be written on the y-axis (use increments of 2g for every box). "Temperature (°C)" should be written on the x-axis (use increments of 10 °C for every 2 boxes).States of Matter Applying like dissolves like For each solute, click the button under the better solvent. Solute I need expert solutions please
- 2. A student makes a standard solution of potassium hydroxide by adding 14.555g to 500.0mL of water. Answer the following questions, being sure to include units and remember sig figs. Show work. a. What is the concentration of this standard solution? b. If the student pours out a 15.6mL sample of this solution, how many moles of sodium hydroxide does the student have in the sample? c. What possible issues many results from air bubbles in the burette for this experiment? Be specific about how this may affect the final calculated concentration of acid (Will it be lower or higher than actual? Why?)Learning Task No. 4: Use the sample problem as a guide to help you solve the % concentration of your prepared solution. Dissolve 10.0g of a substance in 100.0g of water., the concentration by mass will be: Divide the mass of the solute by the total mass of the solution. c%=10.0g10.0g+100.0g* 100%=9.09 Solutions to make: 1. 450 g flour and 1 L water 2. 500 ml alcohol and 1 L water 3. 300 g rice grains and 540 ml water 4. 450 g sugar and 360 ml coconut milk 5. 50 ml liquid detergent and 250 ml waterPlease answer question and just send me the paper solutions dont type the solutions please ASAP Only answer question 9
- A chunk of Zn was breaks down on 200 mL of 0.750 mol/Liter Hydrochloric acid. After that rx, 100 mL of solution is diluted to 400 ml and titrated with 15 ml of 0.250 mol/Liter solution of Sodium Hydroxide until the endpoint. Find the: The exact number of moles of hydrochloric acid in the 200 mL solution Exact number of moles of excess hydrochloric acid which reacted with sodium hydroxide in the 100 mL sampl3 Number of moles of excess hydrochloric acid in the 200 mL solution (first solution) Number of moles of Zn which reacted with hydrochloric acid Mass of the chunk of Zn which was dissolvedSubmit a clean, dry, and properly labeled 50-mL reagent bottle for your unknown solution. Pipet 20.00 mL of the sample in 250-mL Erlenmeyer flask. Add 5 mL of buffer and 5 drops of indicator. Titrate the solution until it turns light blue. If the titration consumes more than 50 mL of the titrant, dilute the sample accordingly. Compute for ppm of CaCO3 using the following table. Mean Molarity = 2.487 x 10^-3 MBlank correction = 0.015 Formula = V (mL) titrant x Mean Molarity of Titrant x Molecular weight of CaCO3 x 1/V (L) sample0.02 M NaOH reagent was standardized using 0.1000 g Potassium hydrogen phthalate (204.22 g/mol) and it required 25.8 mL to reach end point. Answer must be in 4 decimal places.