6. Calculate the number of grams of KBr (formula wt. = 119 u) contained in 120.mL of a 0.720 M solution. a. 14.3 b. 8.64 x 10 -2 c. 10.3 d. 86.4 e. no correct response
Q: 3 attermpts left Check my work Be sure to answer all parts. Starting with a 6.701 M stock solution…
A: Given data: Initial concentration of HNO3 = 6.701 M AAt each stage, 25 mL of solution is diluted to…
Q: (d) a mixture of 49.0 mL of 0.12 M KCIO3 and 30.0 mL of 0.28 M Na₂SO4. Assume the volumes are…
A:
Q: Answer is provided. All I need is solution. Thank you From the following formula or a progesterone…
A: A question based on analytical process that is to be accomplished.
Q: MEQ 3. How many mg of Magnesium Sulfate (MGSO4) should be added to an IV solution to provide 5 mEq…
A: The solution is given below -
Q: How many mL of 6.00 ppm solution are needed to make 4.00 L of a 0.100 ppm solution ? (answer = 66.7…
A:
Q: A. Standardizatlon of thlosulfate solution Trial 1 Trial 2 Trial 3 Initial volume of thiosulfate…
A: Molarity = number of moles of solute / volume of solution We are given data for initial and final…
Q: Problems 1. What is the normality of a solution of H2SO4 if it has a specific gravity of 1.84 and…
A: Hello. Since more than one question has been asked, the first question shall only be answered in…
Q: The distribution coefficient, k = (concentration in hexane/concentration in water), for solute A is…
A: Distribution coefficient of solute (Kd) = 7.5 Initial concentration of A in water = 10 g in 90 mL…
Q: Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.19 2.26 2.39 Molarity…
A: To calculate ,we would use the give data values.
Q: 3:29 1 l LTE If you have 155 mL solution of a 0.762 MFECI, solution, how many moles of FeCl, are…
A:
Q: TRIAL 1 TRIAL 2 TRIAL 3 Wt. of vinegar sample 8.2000 g 8.1000 g 8.2500 g Vol. of vinegar sample…
A: Since you have posted multiple questions, we are entitled to answer the first only.
Q: Calculate the molarity of a solution in which 0.250 moles of solute was dissolved in enough water to…
A: Molarity of the solution can be determined by using the formula given below as; Molarity=Moles of…
Q: How many grams of sodium dichromate, Na2 Cr207, should be added to a 100.0-mL volumetric flask to…
A: First of the given data is collected as: Now, to find the mass of sodium dichromate (Na2Cr2O7) that…
Q: Paolo added 5.8 mL of 4.9 M NAOH to 5.4 mL of 0.89 M HCI. Calculate the concentration, in units of…
A: In the given question we have to calculate the concentration of excess OH- in the resulting…
Q: REPORT SHEET PROCEDURE A: Weight of Water needed (show calculations) Weight of Salt needed (show…
A: Mass of salt present in 100 g of salt solution = 10 g Mass of salt present in 1 g of salt solution =…
Q: A 50.00 (±0.03) mL portion of an HCl solution required 29.71(±0.03) mL of 0.01963(±0.0030) M Ba(OH)2…
A: Given, MHCl=29.71 ml×0.01963 mmol Ba(OH)2ml×2mmol HClmmol Ba(OH)250.00 ml
Q: Trial 1 Trial 2 M of NaOH(aq): Average M of NaOH(aq) from part I M of NaOH(aq): Average M of…
A:
Q: How much 0.7 M CaCl2 solution is required to make 381 mL of a 0.4 M CaCl2 solution? Answer in
A: Here we use the formula M1V1= M2V2.
Q: Result: A. Data Trial 1 Trial 2 Weight of KHP Volume of NaOH Used 17 mL (mL) Normality of NaOH…
A:
Q: How many grams of sodium fluoride should be added to 100,000 L of drinking water containing 0.6 ppm…
A: Concentration of sodium fluoride = 0.6 ppm = 0.6 g/mL (ppm = g/mL) Volume of drinking water =…
Q: Find the number of millimoles of solute
A: The solution of the question is given below:
Q: Fe(OH)3___________ + HNO3___________ → HOH + Fe(NO3)3 How many mL of 0.878 M Fe(OH)3 are required…
A: The given unbalanced chemical reaction is: Fe(OH)3___________ + HNO3___________ → HOH + Fe(NO3)3 How…
Q: If 12.4 mL of a 1.54 M NAOH solution was used to neutralized the nitric acid in a 25.12 mL sample.…
A:
Q: 4. What volume of 0.100 M sulfuric acid is required to neutralize 800.0 mL of 0.200 M KOH? Show your…
A: Applying molarity equation M 1V 1= M 2V2
Q: I need help calculating the percent deviation please. reaction equation - 2 MnO4− + 5 C2O42− + 16 H+…
A: We would use formula of percent deviation to calculate percent deviation in Molarity of KMnO4.
Q: 11- the molar concentration of HNO3 (63.0 g/mol) in a solution that has a specific gravity of 1.42…
A:
Q: A solution is prepared by dissolving 20.5 g of NaOH in 130.0 g of water. The NaOH solution has a…
A: Given: Mass of solute, NaOH = 20.5 g Mass of solvent, water = 130.0 g Density of solution = 1.15…
Q: Sample Problem: A water sample was tested for iron content, but was diluted prior to obtaining the…
A: Given, Volume of solution = 10.0 mL Dilution volume = 100.00 mL Concentration of diluted sample =…
Q: Chemistry Question
A:
Q: Sample Problem: A water sample was tested for iron content, but was diluted prior to obtaining the…
A:
Q: . A 20.0g sample of NaCl was dissolved in 125mL of water (density = 1.00g/mL). Calculate the weight…
A: We are having; 20 g Nacl 125ml water Density of water = 1g/ml Mass of water = volume * Density Mass…
Q: 0.02 M NaOH reagent was standardized using 0.1000 g Potassium hydrogen phthalate (204.22 g/mol) and…
A:
Q: A 5.623 g sample of NaHCO3 is dissolved in enough water to make 250.0 mL of solution. Calculate the…
A: The molar mass of NaHCO3 = Atomic mass of Na + Atomic mass of H + Atomic mass of C + 3 X Atomic mass…
Q: SPasiahnyk FSw 40 SI PARTICIPATION opestar The aqueous solubility of lithium phosphate (Li PO,) is…
A:
Q: REPORT SHEET Trial Volume of Acid used ( mL) 20.0 20.C 1. 0.10 0.10 2. Molarity of acid used (M) 3.…
A: At equivalence point : Equivalents of acid = equivalents of base For monovalent acid and base: moles…
Q: 1. Give possible reasons why the percentage recovery might be low. a.
A: 1) There are some reasons for low percent recovery: The reactants are not completely converted into…
Q: Limiting reagent Calculated mass of excess reagent remaining in the mixture after reaction, g…
A:
Q: hat is the mole fraction of each component of a solution that contains 25g Ca(OH), in 132g of liquid…
A: We are authorised to solve only one question at a time. Please post rest of the questions…
Q: ion of 0.1789 M phosphoric acid is used to standardize an unknown solution of sodium hydroxide…
A:
Q: How many mL of 0.146 M NaC2H3O2 are needed to supply 15.7 g NaC23O2 ? Answer in mL
A: Given that: Molarity of NaC2H3O2 = 0.146M = 0.146mol/L Mass = 15.7g Molar mass of NaC2H3O2 = molar…
Q: Read the volume of the liquid in the 150 Erlenmeyer flask. Estimate the volume to the nearest 5 ml…
A:
Q: Lab Sec. Name Desk No. A. Standardized HCI Solution Molar mass Naaco3 Hao =124.0glmol Calculate the…
A: Volumetric analysis is a type of quantitative analysis that allows us to estimate the amount of…
Q: concentration of a rougly 0.2 mol L-1 ammonia solution (NH3, Kp = 1.8x10-5) was calibrated by…
A: The question is based on the concept of titrations. we are titrating ammonia solution with…
Q: Trial-1 Volume of NaOH in Liters. Moles of NaOH (MxV) Moles of CH,COOH Molar Mass Of CH,COOH (g/mol)…
A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…
Q: Problem 8.39
A: Calculation of the volume of stock solution:
Q: EXPERIMENT 6 PRE-LABORATORY QUESTIONS DETERMINING THE SOLUBILITY OF AN UNKNOWN IONIC COMPOUND NAME…
A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…
Q: What is the mass percent of solute for: 7.6 grams of Na2SO4 dissolved in water to give 87.3 grams…
A:
Q: 20 g of Na2SO4 is dissolved in 60 g in water and density is 2.66 g.cm^-3 . find %w/v and molarity
A: Given: The mass of Na2SO4 dissolved in 60 of water = 20 g The de3nsity of the solution = 2.66 g.cm-3…
6. Calculate the number of grams of KBr (formula wt. = 119 u) contained in 120.mL of a 0.720 M solution.
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
- (a) During the analysis of water sample by argentometric titration, results obtained are as follows: Experiment1 2 3 4 Volume 15.5, 15.2 ,15.1 ,15.4 A)Calculate average deviation and relative average deviation for the given data. (b)Calculate the molecular weight of an unknown acid if 8.5 g of it is dissolved in 200.0 ml of water and requires 50.0 ml of 1.5 M sodium hydroxide for complete neutralization .Figure 1:Experimental results Mass of empty weighing dish,g 2.2522g Mass of weighing dish + CaCl2 · 2H2O,g 6.2540g Mass of CaCl2 · 2H2O, g 4.0018g [Na₂CO₃], mol⋅L−1 0.3330 mol⋅L−1 Volume of the CaCl2 solution used, mL 10.00mL Volume of the Na₂CO₃ solution used, mL 10.00mL Mass of the filter paper + watch glass, g 51.3999g Mass of the filter paper + watch glass + dry product (final), g Weight 1=51.7235g Weight 2=51.7058g Figure 2:Calculated data Mass of dry product, g 0.3059g Moles of CaCl2 used, mol 0.02721mol Moles of Na₂CO₃ used, mol 0.02721mol [CaCl2], mol⋅L−1 0.3330 mol⋅L−1 Limiting reagent Calculated mass of excess reagent remaining in the mixture after reaction, g Theoretical yield, g % yield I need help in my lab. The number of mols of cacl2 and na2co3 gives me the same number. If I need to calculate the limiting reagent, how would I be able to do that if they have…5.35g of salicylic acid added to 7.75mL of methanol followed by 10 drops of sulfuric acid,H2SO4 and the resulting mixture was refluxed for 30 min. If 3.85mL of methyl salicylate were distilled from the mixture. What's the percent yield? Answer to 1 decimal place
- ANSWER ASAP PLEASE The Ca2+ in a 25.00mL of underground powder was titrated with 28.60 mL of 0.01350 M EDTA. Calculate the concentration of Ca2+ in ppm. Round off your final answer to four significant figures.The thiourea in a 1.455 g sample of organic material was extracted into a dilute sulfuric acid solution and titrated with 37.31 mL of 0.009372 M Hg2+ via reaction: 4(NH2)2CS + Hg2+ →[(NH2)2CS]4 Hg2+ P.S. Answer only the last two letters of the following questions. (Only C and D) a. Is this an example of total analysis technique or concentration technique? Explain. b. Calculate the percent (NH2)2CS ( 76.12 g/mol) in the sample. c. What is classification of the analysis based on the amount of sample and amount of analytes present? Explain. d. If the true value is 10.00%, calculate the absolute and relative error.Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 2.29 1.41 1.95 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 50.37 49.39 49.84 Table 2. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 2.29 1.41 1.95 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 50.37 49.39 49.84 Expected color at end point Volume of NaOH used (mL) 48.08 47.98 47.89 Compute for the ff: a. Average moles of acetic acid (mol)? b. Average molarity of acetic acid (M)? c. Average molarity of acetic acid (M)?
- Part B (Trial #1) Part C (Trial #2) Mass of empty evaporation dish 154.48 g 158.34 g Volume of sodium chloride solution added to evaporation dish 10.0 mL 10.0 mL Mass of evaporation dish containing sodium chloride crystals after evaporating the water and drying 154.94 g 159.85 g Determine the average molarity for these two trials.Chemistry 1. If your 10 g sample contains 200 µg H2O, calculate the water concentration of your sample in ppm (i.e., µg water per g of sample)? Do not include units in your numeric answer. 2. Calculate the water content of your tablet sample (specimen) as a % wt/ wt: Given: 4g tablet sample was weighed, and S (= KFR volume consumed by sample during titration) = 6.00 mL Submit your answer to 2 decimal places. Do not include the % symbol; only numeric values allowed in your answer.Sample AnalysisSource of Water sample:Tap Water Molarity of Na2S2O3 1 2 3 0.0243 0.0245 0.0228 Average Molarity of Na2S2O3 0.0239 Trials 1 2 3 Volume of sample used 100.00 100.00 100.00 Final Volume Reading Na2S2O3 (ml) 6.70 10.00 13.10 Initial Volume Reading Na2S2O3 (ml) 3.40 6.70 10.00 Net VolumeNa2S2O3 used (ml) 3.30 3.30 3.10 mg O2 in sample ppm O2 in sample average ppm O2 in sample
- ab experiment by adding drops of KMno4 to a solution of distilled water and Iron (II) ammonium sulfate. I measured the iron ammonium sulfate in grams and added the same amounts into two flasks. I then added 25mL of distilled water and mixed. Then I added 5 mL of H2SO4 (sulfuric acid) into the solution. After that, I slowly added drops of KMno4 until the solution turned a pink color (reached end point). I measured the initial and final volume of KMno4. What would be the balanced equation for this reaction? How can I find the moles of KMno4 solution needed to react with all of the 0.100M FeSO4 solution? How do I calculate the molarity of KMno4?EX 2.Given-> Volume of Na+ = 500 ml Molarity of Na+= 0.0100M Molar mass of Na2CO3 = 105.99 gm/mole Millimole of Na+ = molarity × volume Number of millimole = 0.0100 × 500 = 5 millimole Na2CO3 ---> 2Na+ + CO32- Millimole of Na2CO3 = millimole of Na+/2 Millimole of Na2CO3 =5/2 = 2.5 millimole Mole of Na2CO3 = 2.5 × 10-3mole (1 mole = 10^3 millimole) Weight of Na2CO3 required = mole × molar mass = 2.5 × 10-3 × 105.99 =0.26 gm Hence, 0.26 gm Na2CO3 must dissolve in 500 ml of water.An EDTA solution was prepared by dissolving the disodium salt in 1 L of water. It was standardized using 0.5063 gram of primary standard calcium carbonate (MM: 100.08) and consumed 28.50 mL of the solution. The standard solution was used to determine the hardness of a 2 L sample of mineral water, which required 35.57 mL of EDTA solution. 1. What is the analyte in the analysis? Answer 2. What is concentration (M) of the EDTA solution used in the analysis? Answer 3. What is the concentration (ppm) of CaCO3 in the sample?
