A practitioner will make a titration curve. The practitioner pipetted 10 mL of 0.1 M HCl solution and put it into a clean and dry Erlenmeyer flask. After that, this practitioner prepared a clean burette (size 50 mL), mounted using clamps on a stand. The burette faucet was tightly closed, after being rinsed using 0.1 M NaOH solution. Using a funnel, 0.1 M NaOH solution was added to a scale of 0 mL. Place the Erlenmeyer flask containing the HCl solution just below the tip of the burette (under the faucet). Calculate the pH of the solution in the Erlenmeyer for each addition of a volume of 0.1 M NaOH solution. Make a table consisting of 3 columns (No, mL of NaOH solution added, calculation of the pH of the mixture). Fill in the mL of added NaOH solution ( 0, 1
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A practitioner will make a titration curve. The practitioner pipetted 10 mL of 0.1 M HCl solution and put it into a clean and dry Erlenmeyer flask. After that, this practitioner prepared a clean burette (size 50 mL), mounted using clamps on a stand. The burette faucet was tightly closed, after being rinsed using 0.1 M NaOH solution. Using a funnel, 0.1 M NaOH solution was added to a scale of 0 mL. Place the Erlenmeyer flask containing the HCl solution just below the tip of the burette (under the faucet). Calculate the pH of the solution in the Erlenmeyer for each addition of a volume of 0.1 M NaOH solution. Make a table consisting of 3 columns (No, mL of NaOH solution added, calculation of the pH of the mixture). Fill in the mL of added NaOH solution ( 0, 1, 2, 3, 4, 5, 6, 7, 8, 9; 9.1; 9.2; 9.3; 9.4; 9.5; 9.6 ; 9,7; 9,8; 9,9; 10; 10,1; 10,2; .......etc .
Draw a curve using millimeter block paper (manual) or with the help of an application on a computer, between mL of NaOH solution added (sb x) vs calculated pH (sb y). .
Based on the obtained curve, determine the pH of the equivalence point. (moles of acid = moles of base)!
In the same way, do for 20 mL of 0.1 M CH3COOH sol with 0.1 M NaOH sol; 20 mL of 0.1 M HCl sol with 0.1 M NH4OH soln.
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