A chemistry student weighs out 0.216 g of chloroacetic acid (HCH₂CICO₂) int a 250. mL volumetric flask and dilutes to the mark with distilled water. H plans to titrate the acid with 0.2000M NaOH Solution. Calculate the volume of NaOH solution the student will need to add to reach the equivalence point. Round your answer to 3 significant digits. mL 0

Solubility Based on the strength and type of intermolecular forces between ammonia (shown below) and water (H,O), one would expect ammonia to be in water. H-N-H H. soluble Submit Answer Save for Later not soluble SAMSUNG @ #3 $ & * 2 3 4. 9. W e r y u S d. j k C V in

Solve both parts otherwise I will downvote with explanation

5. Species Y is to be extracted from a 1.00 L aqueous sample using multiple 20.0 mL portions of an extractant (K = 5.1). In order to remove 95% of Y from the sample, what minimum total volume of extractant is required? a) 20.0 mL b) 40.0 mL c) 60.0 mL d) 80.0 mL e) 100.0 mL

please help?

Name: Date: Section: Report Sheet: Determination of Molecular Weight Through Freezing Point Depression Analysis 30 Part A: Volume of Cyclohexane mL Mass of cyclohexane (d =0.7786 g/mL) 6.0 °C Freezing Point of cyclohexane 128 Part B: Molecular Weight of Naphthalene g/mol 0.23 Mass of Sample 1 Moles of Sample 1 Mass of Sample 2 0.18 Moles of Sample 2 Moles m (mol/kg solvent) T,('C) AT, Naphthalene 5.1 TRIAL 1 5.3 TRAIL 2 k, Cyclohexane CC/m) Part C: Unknown Number 0.21 0.19 Mass of Sample 1 Mass of Sample 2 Grams Unknown T,('C) AT 0.21 4.8 TRIAL 1 0.19 5.0 TRAIL 2 Moles UnknownTRIAL 1 (moles) TRIAL 2 (moles) TRIAL 1 (g/mol)TRIAL 2 (g/mol) Molecular Weight Unknown (g/mol) AVERAGE MOLECULAR WEIGHT OF UNKNOWN

part A 1. Concentration of Known NiCl2 Stock Solution ___500________ mM   Tube Number   Blank #1 #2 #3 #4 #5 2. Volume of Known NiCl2 Stock Solution Pipetted Into Tube 0.00 mL 1.50 mL 3.00 mL 4.50 mL 6.00 mL 7.50 mL 3. Volume of Distilled Water Pipetted Into Tube 11.00 mL 9.50 mL 8.00 mL 6.50 mL 5.00 mL 3.50 mL 4. Total Volume of Solution In Tube 11.00 mL 11.00 mL 11.00 mL 11.00 mL 11.00 mL 11.00 mL 5. Diluted Concentration of NiCl2 In Tube ----------- 68.2 mn 136mn 204mn 273mn 341mn 1. Equation for the Best-Fit Straight Line Y=3822x+4.7446 2. Absorbance at λmax for Diluted Unknown 0.87 3. Concentration of NiCl2 in Diluted Unknown 25.693 mM Determine the dilution factor for your diluted unknown U1 based on how you prepared the solutions in Part A. Record this on your report sheet in Part D #4.

Preparation of 0.1 M Sodium Hydroxide Solution   (Answer must be in the format of the second photo)

Please correct answer and don't use hand rating

a. A 1.00 liter solution contains 0.45 moles nitrous acid and 0.35 moles potassium nitrite .If 0.17 moles of hydroiodic acid are added to this system, indicate whether the following statements are true or false.(Assume that the volume does not change upon the addition of hydroiodic acid.) A. The number of moles of HNO2 will decrease. B. The number of moles of NO2- will decrease. C. The equilibrium concentration of H3O+ will remain the same. D. The pH will increase. E. The ratio of [HNO2] / [NO2-] will increase. b.  A 1.00 liter solution contains 0.38 M ammonia and 0.49 M ammonium bromide. If 0.120 moles of barium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of barium hydroxide.)  A. The number of moles of NH3 will decrease.  B. The number of moles of NH4+ will decrease.  C. The equilibrium concentration of H3O+ will increase.  D. The pH will increase.  E. The ratio of [NH3] /…