What's the average concentration of NH3 in the commercial cleaning solution using the data Volume of Cleaning solution 10.00 for all 3 trials, molarity of HCl 0.0530 for all 3 trials, Volume of HCl first trial is 4.8 second trial is 4.4 and third trial is 4.4, Molarity of NH3 in cleaning solution first trial is 0.0254 second trial is 0.0233 and third trial is 0.0233. What's the diluted solution in all 3 trials?
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What's the average concentration of NH3 in the commercial cleaning solution using the data Volume of Cleaning solution 10.00 for all 3 trials, molarity of HCl 0.0530 for all 3 trials, Volume of HCl first trial is 4.8 second trial is 4.4 and third trial is 4.4, Molarity of NH3 in cleaning solution first trial is 0.0254 second trial is 0.0233 and third trial is 0.0233. What's the diluted solution in all 3 trials?
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- A solution of HCl was titrated against sodium carbonate. What is the average normality of acid in the given data? (MW Na₂CO3 = 106) T2 0.3479 0.3562 0.3042 Weight (g) Initial V (ml) 0.80 1.60 35.20 36.70 39.80 Final V (mL) Vol HCl used (mL) 35.10 39.40 N of HCl (eq/L) 0.1954 0.1870 Average N of HCl (eq/L)a) Which salt has minimum solubility at40°C? 200 160 KNO, 180 170 160 b) At what temperature solubility of KCl is 50g in 100g of water? 150 140 130 120 110 100 90 c) How much KCl will dissolve in 125g of 80 water at 10°C? 70 60 KCI 50 40 Naci 30 d) If 70g of KNO; is dissolved in 100g of water At 50°C, find whether solution is saturated, unsaturated or supersaturated? 20 10 20 40 80 80 100 Temperature ("C) Figure 18 Relationship between solute solubility in water and temperature Grams of solute dissolved in 100 g of watera) Which salt has minimum solubility at40°C? 200 100 KNO 160 170 160 b) At what temperature solubility of KCI is 50g in 100g of water? 150 140 130 120 110 100 e) How much KCI will dissolve in 125g of water at 10'C? 70 KCH 40 30 Naci d) If 70g of KNO, is dissolved in 100g of water At 50'C, find whether solution is saturated, 20 10 O 20 40 60 o 100 Temperature ("C) unsaturated or supersaturated? Figure 18 Relationship belween solute solubility in water and temperature Grams of solute dssolved in 100 g of water
- Calculate the percent difference in the two values for the molarity of the NaOH solution by: %Difference =[M1-M2]\Mavg x100% Given: 1st value for the molarity of NaOH = 0.0647 M 2nd value for the molarity of NaOH= 0.2627 M NaOH vs H2SO4 Burette solution is NaOH and the pipette solution is 10.0 mL of 0.205 M H2SO4 Titration Initial burette reading Final burette reading Volume of NaOH consumed Average volume of NaOH Approximate 0.0 mL 31.8 mL 31.8 mL 31.7 mL Titration 1 0.0 mL 31.5 mL 31.5 mL Titration 2 0.0 mL 31.7 mL 31.7 mL To find the average volume Average volume = 31.8 mL + 31.5 mL + 31.7 mL331.8 mL + 31.5 mL + 31.7 mL3 = 31.7 mL NaOH vs CH3COOH Burette solution is NaOH and the pipette solution is 5.0 mL of Vinegar Titration Initial burette reading Final burette reading Volume of NaOH consumed Average volume of NaOH Approximate 0.0 mL 20.1 mL 20.1 mL 20.3 mL Titration 1 0.0 mL 20.9 mL 20.9 mL Titration 2 0.0 mL 20.0 mL…solute 0.147 g C6H7NaO6 molar mass 198.11, dissolves in 50.00 mL, absorbance of solution 0.862, absorbance of standard 0.863 calculate moles of solute, volume of solution (L), %m/v, M, % errorFor results/conclusions Using the images attached Write 2 paragraphs 1st paragraph: Starts with Objective. Results of DeltaT and i stated 2nd paragraph: sources of errors discussed The objective is The colligative properties are the properties that undergo a change when a solute is introduced to a solvent. Freezing point depression is also a colligative property. The addition of a solute to a solvent reduces the freezing point of the resulting solution. The freezing point of the solution is always lower than the freezing point of the solvent. This difference in the freezing point between solvent and solution is called freezing point depression. The freezing point depression is directly proportional to the molality of the solution or the number of moles of solute present in the solution.
- 4- If Ksp of Agl 8.3x10-17 calculate the solubility of Agl by gm/L ? 234. 8 x9. 11x10-6 gm/L O 2.34 8 x9. 11×10-6 gm/L 23.4 8 x9. 11x10-6 gm/LConsider the solubility profile outlined below of acetanilide in water. Solubility in water at 20C 0.50 g/100mL Compound Acetanilide (a) Determine the minimum amount of water in mL required to dissolve 5.5 grams of acetanilide completely at 100 C. Submit your answer without units Submit Answer Tries 0/99 Solubility in water at 1000 5.50g/100 mL (b) If the solution question (a) above is cooled to 20 C, determine the amount in grams of acetanilide that would remain dissolved water. Submit your answer without units. Your answer Submit Answer Tries 0/99 (c) If the undissolved acetanilide in question (b) above is isolated by a filtration method, determine the amount grams that would be recovered and calculate the % recovery of this process [assuming zero material loss during filtration and transfers]. Submit your answer without units. Your answer [% recovery] Submit Answer Tries 0/99 This discussion is closed. Send FeedbConcentration of Acetic Acid in a Vinegar Solution. Average molarity of NaOH Volume HC₂H30₂ sample Final buret reading Initial buret reading Volume NaOH (Show all units and all calculations) Molarity of HC₂H30₂ (unrounded) Average molarity of HC₂H302 (unrounded) Deviations Average deviation Best estimate for molarity of HC₂H302 Average mass percent HC₂H302 46.4mL Oml Ran out of Base ↓ ↓ ↓ ↓ 10.014 HOA je beart giov isults weari?! ferottelucuny Cambia) 10 Kousad Question 1. A Rolaids tablet contains calcium carbonate that neutralizes stomach acid. If 44.55 mL of 0.448 M hydrochloric acid is required to neutralize one tablet, how many milligrams of calcium carbonate are in a Rolaids tablet? CaCO, (s) + 2HCl(aq) → CaCl₂ (aq) + H₂O (1) + CO₂ (g)
- Calculate the molalities of some commercial reagents from the following data: (Assume 100 g of solution.) Data HCl(aq) NH3(aq) Formula weight (g/mol) 36.465 17.03 Density of solution (g/mL) 1.19 0.90 Weight % 31.3 27.0 Molarity 11.9 13.5 Molality of HCl(aq) :_____ Molality of NH3(aq):______For a given electrolyte: Concentration = 0.01 M & g = 0.898 Concentration = 0.05 M & g = 0.800 What is the activity coefficient when Concentration = 0.024 M? G=gammaA solution is prepared by dissolving 11.3 g of Ca(NO3)2 in 115 g of water. The molal freezing point depression constant for water kf, is 1.86°C/m and the molal boiling point elevation constant for water kb, is 0.512°C/m. The change in the boiling point of the solvent when Ca(NO3)2 was added is __________ OC. The freezing point of the solvent depresses by __________ OC. The freezing point of the solution is __________ OC.