The buret, used for titrations, has graduations of 0.1 ml; therefore, the readings should have ___ decimal places.
Answer:-
The buret has the graduations of 0.1 mL its means the there are 10 graduation in 1 mL . so, the reading should have 1 decimal place .
So, 1 is correct answer.
It is also its least count.
The buret, used for titrations, has graduations of 0.1 ml; therefore, the readings should have ___...
Group 4 - Titration Data Titration with 10 ml of 0.1 N oxalic acid, used 12.5 mL NAOH solution. Please calculate the concentration of these solutions and post the details of your calculations and final results so I can check them. Titration Data was measured with a 50 mL burette with graduations of 0.1 mL. All other reagents were measured with a 5 mL pipette with graduations of 0.1 mL. Your reagents are labeled Group 4
Answer questions regarding buret a) What is a buret card and how is it used? b) When using a 50 mL buret as shown in the pictures, to what decimal place should a buret be read? c) List two ways to remove bubbles in the tip of a buret?
Sodium hydroxide is used extensively in acid-base titrations because it is a strong, inexpensive base. A sodium hydroxide solution was standardized by titrating 36.78 mL of 0.1143 M standard hydrochloric acid. The initial buret reading of the sodium hydroxide was 1.52 mL, and the final reading was 39.50 mL. What was the molarity of the base solution?
QUESTION 2 Suppose you have 20 mL of 0.1 M HCl. What will the pH of the solution be after 10 mL of 0.1 M NaOH is added? Report your answer to 2 significant figures (i.e., 2 decimal places). Suppose you have 20 mL of 0.1 M HCl. What will the pH of the solution be after 30 mL of 0.1 M NaOH is added? Report your answer to 2 significant figures (i.e., 2 decimal places).
Constant-boiling HCl can be used as a primary standard for acid-base titrations. A 50.00 mL sample of constant-boiling HCl with a concentration of 0.1225 M was collected and titrated to an end point with 35.60 mL of Ba(OH)2 solution. What is the molarity of the Ba(OH)2 solution?
Constant-boiling HCl can be used as a primary standard for acid-base titrations. A 50.0 mL sample of constant-boiling HCl with a concentration of 0.1166 M was collected and titrated to an end point with 37.17 mL of Ba(OH)2 solution. What is the molarity of the Ba(OH)2 solution?
This problem deals with Acid-base titrations and pH scale for a weak acid and a weak base. Calculate the pH of the solution that results from adding 7.5 [ml] of Ammonia (NH3) to a beaker that contains, 100 ml of distilled water and 15 ml of 0.1 M Acetic acid (HC2H3O2). A buret containing 50 mL of 0.1 M Ammonia (NH3) is being used as the titrant. The beaker containing 100 ml of distilled water, and 15 ml of 0.1...
Constant‑boiling HClHCl can be used as a primary standard for acid–base titrations. A 50.00 mL50.00 mL sample of constant‑boiling HClHCl with a concentration of 0.1051 M0.1051 M was collected and titrated to an endpoint with 34.91 mL34.91 mL of a Ba(OH)2Ba(OH)2 solution. What is the molarity of the Ba(OH)2Ba(OH)2 solution?
Monitosing.Acid-Base Titrations wih a pH Meter 3. student titrated 20.0 mL of 0.410M HCI with 0.320M NaOH and collected the following data. Pre-Laboratory Assignment 1. Briefly explain: (a) why you must use caution when with HCI solutions 0.32 A working volume NaOH solution added, mLpH 0.39 0.46 0.54 0.62 0.70 0.78 0.87 0.96 1.07 1.19 1.35 1.56 1.93 2.09 2.35 3.06 11.40 11.80 12.00 12.20 12.30 0.00 2.00 4.00 6.00 8.00 10.00 12.00 14.00 16.00 18.00 20.00 22.00 24.00 24.50...
Acid-base titrations. You have 60.0 mL of a weak base (0.0305 M) and titrate it with a strong acid (0.0500M). pKa of the weak conjugate acid is 4.36. a) What is the pH before the acid is added? b) What volume of the acid is needed at the equivalence point (in mL)? c) What is the pH at the equivalence point? d) What is the pH after 5.00 mL of the acid is added beyond the equivalence point?