Give detailed Solution...give correct answer

e courses.hayden-n stry 1302A/B Discovering... OWL : CHEM 1302B 004 FW20: Chapter 3 Ten mL of a stock solution of the bromocresol green indicator is mixed with 10 mL of NaOH. Which of the following is true? Select one: a. The concentration of the indicator increases. b. The concentration of the indicator decreases. c. The concentration of the indicator remains the same. d. None of the above. For this experiment, what will be typed into the MicroLab unit instead of the concentration of the indicator? Select one: a. The concentration of NaOH. b. The concentration of hydronium [H3O`]. c. The concentration of HIn. d. The concentration of In.

A solution containing 78 g of NaOH in 2750 mL of water would have a pH of? I keep coming up with pH = 13.9 but the answer sheet says 5.85....not sure what I'm doing wrong?

How do I solve this? I do know that it is linear.

can search the web by typing the chemical name followed by SDS) b) what is the best practice to follow if a small amount of sulfuric acid (1M) comes in contact with your bare hand? 2. Write a one or two sentence statement of what the purpose of this lab is. 3. To prepare for laboratory: For each of the eight unknowns solutions that you will identify in lab (see above or table below), identify the chemical color and the pH category (acidic, neutral, or basic) that you expect to find. Prepare a table to summarize your initial expectations for the color and pH tests. A. Introduction- A Fictitious Scenario ne Chem-Police, a division of the Office of Homeland Security created in re-

Simulation illustrates how buffers work.?What type of buffer is presented simulation? Acidic or basic? What is the role of the buffer solution?

Example Problem: Consider The Titration of 100.0 mL of 0.200 M CH3NH2 by 0.100 M HCl. Calculate The pH After 65.0 mL of HCl Added. (Kb for CH3NH2 = 4.4 x 10^-4): a. 10.96. b. 9.75. c. 7.00. d. 3.68. e. 2.54.

Mm.12. Subject:- Chemistry  ...

- If the concentration of the hydroxyl ion (1-OH) in the solution is (0.0001) molar, then the value of the acidity function (PH) of the solution •..• •.

Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula K5 1.8 x 10-5 4.38 x 10-4 5.6 x 10-4 3.8 x 10-10 1.7 x 10-9 Ammonia NH3 Methylamine Ethylamine Aniline Pyridine CH;NH2 CH;NH2 C,H;NH2 C;H;N NH,* CH;NH3* CH;NH;* CH;NH;* C3H;NH*