Imagine you were the student lab prep assistant for a Chemistry Lab and you needed to provide a standardized solution of NaOH. How would you standardize a solution before putting it out for other students to use?
standardized solution of NaOH :
Standardization is a process of determining the exact concentration (molarity) of a solution. Titration is the analytical procedure often used in standardization.
The endpoint is determined using an indicator : indicates (signals) the endpoint. The indicator used in this experiment is phenolphthalein.
This experiment involves simple acid-base titration. In this the molarity of a sodium hydroxide solution (NaOH) is determined by titrating a known sample of potassium acid phthalate (KHP; HKC8H4O4) with the NaOH.
Imagine you were the student lab prep assistant for a Chemistry Lab and you needed to...
Suppose that the lab prep staff incorrectly recorded the masses of KHP. You are told they used 0.50 g of KHP to standardize the NaOH solution; however, they actually used 0.10 g KHP in the standardization. What will this do to your calculated concentration of the unknown HCI solution? Explain your answer.
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.70. You have in front of you 100 mL of 6.00×10−2M HCl, 100 mL of 5.00×10−2M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your error, you...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.40. You have in front of you 100 mL of 6.00×10−2 M HCl, 100 mL of 5.00×10−2 M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.50. You have in front of you 100 mL of 7.00×10−2 M HCl, 100 mL of 5.00×10−2 M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.80. You have in front of you 100 mL of 7.00×10−2 M HCl, 100 mL of 5.00×10−2 M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.40. You have in front of you 100 mL of 6.00×10−2M HCl, 100 mL of 5.00×10−2M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your error, you...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.80. You have in front of you 100 mL of 7.00×10−2mol L−1 HCl, 100 mL of 5.00×10−2mol L−1 NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...
Constants Periodic Table Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.80. Part A You have in front of you 100 mL of 7.00x10-2 MHCI, 100 mL of 5.00x10-2 MNaOH, and plenty of distilled water. Assuming the final solution will be diluted to 1.00 L , how much more HCl should you add to achieve the desired pH? Express your answer to three significant figures and include the...
chemistry
1. Your boss asks you to prepare and then standardize a sodium hydroxide solution, which you do as you did in this lab. The average concentration is 0.1063M. He then hands you a solution of nitric acid and asks you to titrate it with your NaOH solution. It requires 27.33mL of your tandardized NaOH solution to titrate 24.79mL of the nitric acid solution. Write a chemical quation for the neutralization reaction and then calculate the molarity of the nitric...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.40. You have in front of you 100 mL of 7.00×10−2 M HCl, 100 mL of 5.00×10−2 M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...