(1)A primary standard is reagent which is very pure. This standard is a reference chemical used to measure an unknown concentration of another known chemical.
(2) Mass of oxalic acid dihydrate = 2.471 g
Molar mass of oxalic acid dihydrate = 126.065 g/mol
Number of moles of oxalic acid dihydrate = Mass in gram / Molar mass = 2.471 g / 126.065 g/mol = 0.0196 mol
Volume of solution = 250.0 ml = 250.0 L / 1000 = 0.250 L
Molarity = number of moles of solute / Molar mass
Molarity = 0.0196 mol / 0.250 L = 0.0784 mol/L = 0.0784 M
(3) A secondary standard is a standard that is prepared in the laboratory for a specific analysis. It is generally standardized against a primary standard.
(4) Concentration of NaOH = 6 M = 6 mol/L
Volume of NaOH solution = 9 ml = 9 L / 1000 = 0.009 L
Number of moles of NaOH = 6 mol/L * 0.009 L = 0.054 mol
Final volume of solution = 500 ml = 500 L / 1000 = 0.500 L
Molarity of the base = 0.054 mol / 0.500 L = 0.108 mol/L = 0.108 M
- What is a primary standard? You have weighed out precisely 2.471 g of oxalic acid...
Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the unwieldy formula of KHC8H4O4. This is often written in shorthand notation as KHP. If 37.5 mL of a sodium hydroxide solution are needed to neutralize 2.14 grams of KHP, what is the molarity of the sodium hydroxide solution? __________M Oxalic acid dihydrate is a solid, diprotic acid that can be used in the laboratory as a primary standard. Its formula...
Data Table 1 Mass of flask and oxalic acid (g) 117.43 Mass of empty flask (g) 116.93 Mass of oxalic acid (g) 0.5 Moles of oxalic acid (mol) Final volume of NaOH (mL) 17 Initial volume of NaOH (mL) 5 Volume of NaOH used (mL) 12 Moles of NaOH (mol) Molarity of NaOH (M) Data Table 2 Mass of flask and vinegar (g) 126.61 Mass of empty flask (g) 121.63 Mass of vinegar (g) 4.98 Final volume of NaOH (mL)...
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 201.mg of oxalic acid H2C2O4 , a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 63.0mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide...
molarity of acid: 0.1435M volume:25ml 1. Use the molar mass and moles of acetic acid to determine the mass of the acetic acid in the 25.00-ml sample. 2. Calculate the mass/volume percentage (m/v %) by dividing the mass of acetic acid in grams by the volume of the vinegar sample in mL and multiplying by 100. 3. For the reaction of sodium hydroxide solution with a solution of hydrochloric acid: a. Write a balanced molecular equation for the reaction, including...
informations to solve the problem supooosed 3.109 g of sodium hydroxide was weighed out,dissolved, quantitively transferred to a 250 ml volumetric flask, made up to the mark,and mixed well, what is the molarity of sodium hydroxide? the answer is 0.3109 M 1.a. Burets are used to transfer titrant in a titration. A burette is depicted in the lab manual. A 10.00 mL sample of vinegar was titrated with the sodium hydroxide sample from question 1. The initial volume of sodium...
ELIMINARY EXERCISES: Experiment 16 Acid-Base Titrations- Define the following terms associated with titrations: a. standard solutions are base Soluchon When the molanty is alrea known. b. ondpoint is the pant at which color change occurs. C. indicator quie. Watersplutte dues that have one color in basic. 2. Write the balanced formula equation and the net ionic equation for the reaction of sodium hydroxide with hydrochloric acid. Formula equation: Net Ionic equation: 3. What is the molarity of a solution prepared...
20.5 g of chromic acid are dissolved in a 250 mL volumetric flask. a) what is the concentration of the solution? b) If 10.1 mL of the solution in a) is diluted with 75.5 mL of water, what is the resulting concentration? c) If 20.5 mL of the chromic acid solution in a) are titrated with 25.0 mL of sodium hydroxide solution, what is the molarity of the NaOH solution? (need balanced equation)
20.5 g of chromic acid are dissolved in a 250 mL volumetric flask. a) what is the concentration of the solution? b) If 10.1 mL of the solution in a) is diluted with 75.5 mL of water, what is the resulting concentration? c) If 20.5 mL of the chromic acid solution in a) are titrated with 25.0 mL of sodium hydroxide solution, what is the molarity of the NaOH solution? (need balanced equation)
You want to determine the concentration of acid in a particular solution. To this end, you decide to titrate the acid with a standardized sodium hydroxide solution. You quickly throw together an approximately 0.1 M NaOH solution, and then you realize you need to know the exact concentration of this solution before you can use it for anything meaningful. 1. Using an acid-base titration, 30.65 mL of your NaOH solution were needed to neutralize 0.6923 g of KHP (potassium hydrogen...
Questions 1. Calculate the molarity of a sodium hydroxide (NaOH) solution that is titrated with 0.6887 g of oxalic acid (Equation 2). The titration requires 15.80 mL of the NaOH solution to reach the end point. Calculate the molarity of a sulfuric acid (H,SO) solution if 30.10 mL of 0.62 10 M NaOH is required to reach the end point when titrated against 10.00 mL of the unknown acid solution. The balanced chemical equation for the reaction is given below....