Act B3_SOLN-SI_S2023_LabReport_Template

Find the Final volume of buret (mL) and the Concentration of NaOH (M )

CHM 17 Experiment #8   CONCENTRATION OF A SOLUTION   Discussion   This virtual experiment involves the determination of the conc­entration of salt (sodium chloride, NaCl) in an aqueous solution.  Concentration may be expressed many ways, and this experiment studies two systems: molarity (M) and weight/volume percent (%w/v).   Molarity is defined as the number of moles of solute (in this case NaCl) in a liter of solution. It is calculated with the following equation:                                                   M = moles solute                                                                 liters solution                                      Percent concentration (w/v) is defined as the number of grams of solute (in this case NaCl) in 100. mL of solution. It is calculated with the following equation:                                             %(w/v) =  grams solute  x  100                                                             mL solution   The experimental method…

Help with the CHEM Lab report please! It is about Volumetric Analysis  There is also a Burn trail please make sure for that!

10:00 A l 5G | Question 6 of 15 Submit What mass grams of nitric acid , HNO3, is required to neutralize (completely react with) 4.30 g of Ca(OH)2 according to the acid-base reaction: 2 HNO:(aq) + Ca(OH)2(aq) → 2 H20(1) + Ca(NO3)2(aq) X STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 74.10 3.60 mol Ca(OH)2 18.02 0.0682 g H20 2 164.10 mol Ca(NO3)2 6.022 x 1023 0.0580 g HNO3 4.30 0.116 mol H20 1 mol HNO, 7.31 g Ca(ОН)2 63.02 g Ca(NO3)2 Tap here or pull up for additional resources

Ca2+ in a drinking water sample was analyzed by the following reactions below: Ca2+(aq) + C2O42-(aq) → CaC2O4 (s) → CaO(s) + CO(g)+ CO2(g) First an excess of C2O42- was added to 0.10 L of the Ca2+ water sample. Then CaC2O4 was precipitated, which was demcomposed into CaO with filtering and some heat. The CaO was measured to be 5.61 mg. What is the concentration of Ca2+ in the original water sample? The MW of CaO is 56.1 g/mol.      0.0100M     0.0010 M     1.00 M     0.100 M   The partition coefficient (K) of methylamine (CH3NH2) is 4.50, preferring the organic layer over the aqueous layer in this extraction. The Ka of methylammonium (CH3NH3+) is 2.00 x 10-11. If 10 mL aqueous methylamine solution at pH 11.0 is extracted with 20.0 mL organic solvent, what is the fraction of solute remaining in the water (q)?   HINT: methylamine is a weak base.     14.3%     10.0%     18.2%     81.8%

How many grams of nitric acid , HNO3, are required to neutralize (completely react with) 4.30 |g of Ca(OH)2 according to the acid-base reaction: 2 HNO3(aq) + Ca(OH)2(aq) – 2 H20(1) + Ca(NO3)2(aq) STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 1 6.022 x 1023 0.116 74.10 164.10 0.0580 4.30 0.0682 3.60 18.02 7.31 63.02 |g Ca(ОН)2 mol HNO3 g Ca(NO3)2 mol H20 g HNO3 g H20 mol Ca(NO3)2 mol Ca(OH)2 App Store

You dilute the river water 10 times for the analysis of SDS concentration. The instrument measures an average molar concentration of SDS in the diluted river water to be 1.689 10-4 mol/L. The molar mass of SDS is 288.4 g/mol. What is the mass concentration of SDS in the original river water? 4.87 10-1 g/L 4.87 102 g/L 5.86 106 g/L 5.86 10-5 g/L

The solubility product Kap for AgaPO4 is 3.1 x 10 18. What is the solubility of silver phosphate in a solution which also contains 0.23 moles of silver nitrate per liter? Report your answer in scientific notations with ONE place past the decimal point. Use this format: 1.2*10^-3 Do not add units in your answer, Type your answer...

AR TIT Concentration (grams/kg H₂O) Graph 2: Solubility Curve for Sodium Nitrate (NaNO3) 2000 1800 1600 1400 1200 1000 800 600 400 200 0 0 10 7 8 9 10 20 30 40 50 60 70 80 90 100 Temperature (Celsius) What is the maximum amount of NaNO3 that can be dissolved into 1 kg of water at 20° C? What is the maximum amount of NaNO3 that can be dissolved into 1 kg of water at 80° C? If you try to dissolve 1200 g of NaNO3 into 1 kg of water at 70⁰ C, will all of the NaNO3 dissolve? If you try to dissolve 1000 g of NaNO; into 1 kg of water at 20° C, will all of the NaNO3 dissolve? BLIVEWORKSHEETS

attached is a lab. I have all the answers. Can someone just write a nice introduction for this lab for me!! thank you

Pls help ASAP ON ALL ASKED QUESTIONS PLS PLS

Based from the given problem, What is the Normality of the sodium hydroxide solution?

CONCENTRATION DETERMINATION Buret contains NaOH solution *Sodium hydroxide solution: To 1 part reagent grade NaOH add 1 part distilled, carbon dioxide-free water by weight Erlenmeyer flask contains about 9ml of the acid and about 10 ml of distilled water made recently free from CO2 by boiling. DATA SHEET II Final Reading HCI Initial Reading HCI 9.4 Final Reading NaOH Initial Reading NaOH 10.65 10.55 1 ml HCI 1 mL NAOH mL NAOH mL NaOH mL HCL mL HCL Mean Values: 1 ml HCI = 1 mL NaOH = _mL NaOH mL HCL COMPUTATION:

No plagiarism Please! Station #6  =  HClO4 (aq) For this acid, what does the white bead represent?________ blue bead? __________             3rd Color Bead? _________ Record your observations in the particulate drawing. How many acid molecules have broken into ions?  Determine the % ionization for the acid. Write the ionization reaction for this acid.                          ________ → ______ + _______

4 Fill out the rest of the reaction table in a synthesis of Aspirin for salicylic acid.

A student uses TLC to monitor the progression of the reaction from question 1. After 30 minutes, the student develops the plate (right). Lane A = salicylic acid, Lane B = salicylic acid and reaction mixture, Lane C = reaction mixture. What does the student need to do next? A B C

Can you help me filling all the  table with this data please I really appreciate it! Titration of Acetic Acid and Vinegar - Topic

Suppose a student performs a similar reaction using sodium bicarbonate (NaHCO3) instead of sodium carbonate. The sodium bicarbonate is dissolved in water, and a solution of 6.0 M HCl is added to the sodium bicarbonate in increments. Bubbles are observed during the reaction. The data collected is shown in the table. moles of NaHCO3: mass of empty beaker (g) moles of NaCl: mass of beaker and NaHCO3 (g) initial volume of 6.0 M HCl (mL) How many moles of NaHCO3 were used? balanced equation: final volume of 6.0 M (ml) mass of beaker and NaCl (g) How many moles of NaCl were produced by the reaction? Write the balanced chemical equation for the reaction. Include physical states. 84.000 g 86.279 g 20.0 mL 12.0 mL 85.585 g mol mol

H C 2 H 3 O 2 ( a q ) + N a O H ( a q ) ⟶ N a C 2 H 3 O 2 ( a q ) + H 2 O ( l )   Trial  Vi (mL) Vf (mL) 1 4.42 13.88 2     3       For their first trial, a student pipettes 5.00 mL of a vinegar solution into an Erlenmeyer flask. The student titrates the vinegar with standardized NaOH with a molarity of 0.378 M. The volume of titrant used was recorded in the table above. Calculate the molarity of the vinegar solution for this trial. Enter a number without units.

Either sulfuric acid or bismuth(III) nitrate pentahydrate can catalyze this reaction. What is an advantage to using sulfuric acid? What is an advantage of using the bismuth compound?

using table 1, answer the questiosn below.  Mass of Crushed Antacid (g) .500g Concentration of HCl (M) 1.0 M Volume HCl (mL) 5.01ml Concentration of NaOH (M) 1.0M Initial NaOH Volume (mL) 4.10ml Final NaOH Volume (mL) 2.60ml Total Volume of NaOH Used (mL) 1.5ml   HCl available for neutralization (g): Moles of NaOH required to reach stoichiometric point (mol): HCl neutralized by antacid (g): HCl neutralized per gram of antacid (g):

In a terrible accident, a solution consisting of 2.37 kg of nitric acid, HNO3, was spilled on the lab floor. Very quickly, you decide to throw 2.00 kg of sodium carbonate, Na2CO3, on the spilled acid. You then run out of the building due to the significant quantities of carbon dioxide that would form due to the reaction. As you stand outside, you wonder, "Did I add enough sodium carbonate to neutralize the acid?". a) Did you add enough sodium carbonate to neutralize the acid? Yes Ο No b) In the event that you did not add enough sodium carbonate, how much extra would be needed to completely neutralize the acid? If you have added enough, please enter a value of 0 (zero). Needed 0 c) In the event that you did add enough sodium carbonate, how much extra did you add? If you didn't add any extra, please enter a value of 0 (zero). Excess 09 g g

Details Preparation of Dilute Table Solution Molarity of I₂ Standard Solution Molar Mass (g/mole) Ascorbic Acid Number of Tablets per Analysis Mass (g) Container plus 1 Tablet Mass (g) Container less 1 Tablet Mass (g) of 1 Tablet Volume (mL) of Dilute Tablet Solution Titrimetric Analysis of Dilute Tablet Solution Volume (mL) of Aliquot Portion of Dilute Tablet Solution Titrated Final Buret Reading (mL) Initial Buret Reading (mL) Volume (mL) I₂ Solution Delivered No. of mmol 1₂ Reacted No. of mmol Ascorbic Acid in Aliquot Total No. of mmol Ascorbic Acid Present in the Volumetric Flask Total Mass (mg) of Ascorbic Acid Present in 1 Tablet Average Mass Ascorbic Acid/Tablet Deviation Standard Deviation Coefficient of Variation (%RSD) Reported Composition of Tablet Trial 1 50.00 11.64 0.20 0.02512 M 176.14 1 12.2546 11.7824 0.4722 250.00 Trial 2 50.00 22.80 11.64 Trial 3 250 mg Ascorbic Acid/Tablet 50.00 11.20 0.00 mg Ascorbic Acid/Tablet

Suppose a group of volunteers is planning on building a park near a local lake.the lake is known to contain low levels of arsenic .Therefore prior to starting construction the group decides to measure the current level of arsenic in the lake.a) If a14.7cm3 Sample of lake water is found to have 168.3 gems mg Aersinic .What is concentration of arsenic in the sample in parts per billion ,assuming density of lake water is 1.00g/cm3