A beaker contains a 25 mL solution of an unknown monoprotic acid that reacts in a 1:1 stochiometric ratio with NaOH. Titrate the solution with NaOH to determine the concentration of the acid. Perform a titration by setting the concentration of the NaOH solution and adding it to the acid solution using the different Add Base buttons. The equivalence point of the titration is passed when the solution color changes. The unknown sample can be titrated multiple times by pressing the Retitrate button and starting over. Enter the concentration of the unknown acid solution.
Since you have not provided any intial concentration of the NaOH solution, thus I assume that the concentration is 'S'.
Let us now take the volume of NaOH as 25 mL and the unknown acid solution also has the volume of 25mL. So the concentration of the unknown now can be written as = 25×S/25.
Thus NaOH concentration is the new concentration. If amount of NaOH is not exactly 25 mL then you can find out what it exactly is by titration.
I have just shown the calculation procedure since you have not provided any values!!
A beaker contains a 25 mL solution of an unknown monoprotic acid that reacts in a...
A beaker contains a 25 mL solution of an unknown monoprotic acid that reacts in a 1:1 stochiometric ratio with NaOH. Titrate the solution with NaOH to determine the concentration of the acid. Perform a titration by setting the concentration of the NaOH solution and adding it to the acid solution using the different Add Base buttons. The equivalence point of the titration is passed when the solution color changes. The unknown sample can be titrated multiple times by pressing...
NaOH solution Add Base 1.00 ml 0.10 mL Base Added 10.10 ml 0.05 mL Experimental Settings Indicator Methyl orange [NaOH] = 0.50 M • Phenolphthalein Thymolphthalein Set (NaOH), choose an indicator, and add base in increments using the buttons above Retitrate Unknown acid solution 25 ml 1 of 1 The flask contains 25 mL of an unknown diprotic acid aqueous solution that reacts in a 1:2 stochiometric ratio with NaOH. Titrate the solution with NaOH to determine the concentration of...
35.25 mL of NaOH solution are required to titrate 0.5745 g of an unknown monoprotic acid. Prior standardization of the NaOH determined its concentration as 0.1039 M. 1. Use the data provided to determine the molar mass of the unknown acid 2. If 20 mL of a 1.0 M solution of the unknown monoprotic acid is placed into a beaker and 10 mL of 0.1 M NaOH is added, the pH of the final solution is 1.9. What is the...
1) A solution of a weak monoprotic acid of unknown concentration was titrated with 0.23 M NaOH. If a 100.-mL sample of the acid solution required exactly 10. mL of the NaOH solution to reach the equivalence point, what was the original concentration of the weak acid? 2) During the titration on problem (2B), after 5.0 mL of NaOH addition, the pH = 3.68. What is the Ka of the weak acid? please show steps i have an exam tomorrow
A sample of 0.2140 g of an unknown monoprotic acid was dissolved in 25.0 mL of water and titrated with 0.0950 M NaOH. The titration required 30.0 mL of base to reach the equivalence point, at which point the pH was 8.68. a) What is the molecular weight of the acid? b) What is the pKa of the acid?
Questions 3, 4, & 5 pls (3) You will titrate a solution of an unknown acid (HX(aq)) by adding NaOH(aq). Suppose that 25 mL of 0.5 M NaOH(aq) is needed to reach the equivalence point. How many moles of HX were present initially? Show the calculation. (4) You will titrate acid solutions by adding 0.2-0.3-mL or 2-3-mL portions of NaOH(aq). When should you add the smaller volume? (5) The concentration of an aqueous solution of NaOH cannot be accurately determined...
What is the concentration of 25.00 mL of an unknown monoprotic acid if 18.24 mL of standardized 0.125 M sodium hydroxide solution was required to reach the equivalence point of the titration?
If it takes 32 mL of 0.1M NaOH to fully titrate 20mL of an unknown monoprotic acid, what was the initial concentration of an unknown acid before titration.
A beaker is filled with 200.0 mL of a sodium hydroxide solution with an unknown concentration. A 0.0100 M solution of HCl is used in the titration. The equivalence point is reached when 18.5 mL of HCl have been added. What is the initial concentration of NaOH in the beaker?
A 25.0 mL analyte is made up of 0.230 g of an unknown monoprotic acid. The equivalence point is reached after 22.5 mL of a 0.050 M NaOH solution is titrated into the analyte. Based on the following determine a. The initial concentration of the unknown acid. b. The molar mass of the unknown acid. Please show all steps and work!! I am so confused