Molarity is the number of moles of solute present in one litre of solution.
Weight of solute is given by
Given that Molarity of HCl = 12.1 M
Weight of HCl = 12.1 * 100 * 36.5/1000
= 44.17 grams
2) When added base is splashed on the walls of the flask, more amount of base required to neutralize the given volume of acid. The concentration of acid is higher than the theoretical value.
M1V1/n1 = M2V2/n2
M2 = M1*V1*n2/n1*V2
Since V1 is the volume of the base and other parameters are same, concentration of resultant acid is higher than the actual value.
2. Calculate the number of grams of HCI in 100.0 mL of concentrated HCl which is...
Titration of a Weak Base Prelaboratory Questions 1. Will addition of HCl to a solution make it more acidic or more basic? Will the pH increase or decrease? How does an end point differ from an equivalence point? 2. were titrated with a standard HCl solution: 3. Aliquots of an unknown tris sample Use the balanced equation to set up the string calculation showing how the tris a. mol of acid, L of acid. mo of base, and L of...
An acid-base titration is performed: 250.0 mL of an unknown concentration of HCl(aq) is titrated to the equivalence point with 36.7 mL of a 0.1000 M aqueous solution of NaOH. Which of the following statements is not true of this titration? A. At the equivalence point, the OH−concentration in the solution is 3.67×10−3 M. B. The pH is less than 7 after adding 25 mL of NaOH solution. C. The pH at the equivalence point is 7.00. D. The HCl...
Determine how many liters (l) of stock HCl were used in titration #1. Please fill all questions under "Data Analysis" Page 1 is just instruction for Page 2 EXPT 10: TITRATION OF STRONG ACID WITH STRONG BASE Note to Students: when you see the symbol (), this means there is something you must add into the mock data yourself. You may handwrite or type your answers directly on these pages for submission to a Blackboard link. Remember to show all...
a. Calculate the volume of 0.450 M Ba(OH), which will be needed to neutralize 46,00 mL of 0.252 M HCI. b. Find the molar concentration of a sulfuric acid solution, 35.00 mL of which neutralizes 25.00 mL of 0.320 M NaOH. (Careful! Sulfuric acid is diprotic!) c. Calculate the "molarity of water" H₂O in pure water at 30°C. (Hint: The density of water at 30°C is 0.9957 g/mL.] d. A 15.00 mL sample of a solution of H₂SO₄ of unknown concentration was titrated with...
4. A volume of 30.0 mL of 0.10 M NH, (aq) is titrated with 0.20MCThe value of the base-dissociation (aq) constant, K, for HCO2 in water is 1.2 x 1010 at 25°C. a. (1 pt.) Write the ionic equation for the reaction of NH, (aq) with HCL(aq) (1 pt.) What is the volume of base added at the equivalence point? Show work or reasoning. b. (1 pt.) Will the pH of the equivalence point be higher than, lower than or...
STR Data Standard solution: NaOH concentration 025M volume of initial NaOH buret reading final NaOhH buret readingG TUTHL volume of NaOH used Concentration of HCI Calculations(Show all work and remember your units and significant figures) Determine the Molarity (concentration) of HCl using the data you collected and the titration formula. (The concentration of the NaOH used was 0.25M) Record your answer on your data form. Questions 1. State the purpose of this experiment The ouredse of thrs expetmeot bn of...
please answer all parts!! thank you dotiudiculiududuut 2 30 Consider the buret above, If before starting the titration, the buret was read at 0.10ml NaOH, how many mls of NaOH have been added? ס 30 . 00 O 30.10 28.80 29.00 Bududududude A titration was performed with 0.100M NaOH and a weak acid of unknown concentration. Initially the buret was filled to 0.10ml 0.10ml, before the start of the titration. The figure above shows the buret at the endpoint. How...
Data Standard solution: NaOH concentration 0.25 M Volume of HCl used (Va) Initial NaOH buret reading Final NaOH buret reading Volume of NaOH used (Vb) Concentration of HCl (Ma) 10.00 ml 2.00 ml 16.10 ml 14.10 ml Determine the Molarity (concentration) of HCI using the data you collected and the titration formula. (The concentration of the NaOH used was 0.25M) Record your answer on your data form. United States Focus 17. It takes 75ml of a 2.5M HCl solution to...
Concentration of NaOH = 1600 x10- Molar Sodium hydroxide Nach Trial 1 Trial 2 Trial Trial 4 2.60/1.20 11.40/1.30 28.20 29.10.26.1026.50 Initial buret reading Final buret reading Volume of NaOH added Moles of NaOH added Moles of HCl reacted Molarity of diluted HCI Molarity of undiluted HCI Average molarity of undiluted HCI Precision PROCEDURE 1. Obtain approximately 40 mL of an unknown acid in an Erlenmeyer flask from your teaching assistant. 2. Clean your 250-ml volumetric flask (contains exactly 250.00...
Concentration of NaOH = 1600 x10- Molar Sodium hydroxide Nach Trial 1 Trial 2 Trial Trial 4 2.60/1.20 1.40/1.30 28.20 29.10.26.1026.50 Volume of NaOH added Initial buret reading Final buret reading Moles of NaOH added Moles of HCl reacted Molarity of diluted HCI Molarity of undiluted HCI Average molarity of undiluted HCI Precision PROCEDURE 1. Obtain approximately 40 mL of an unknown acid in an Erlenmeyer flask from your teaching assistant. 2. Clean your 250-ml volumetric flask (contains exactly 250.00...