take a 25.00 mL sample of 0.150 M hypochlorus acid and to it add 10 mL of 0.130 M NaOH. What is the resultant pl of the solution, given that hypochlorus acid has a Ka = 2.9 × 10 ^ - 8?

An analytical chemist weighs out 0.203 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1500M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 18.0 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. mol Explanation Check 0.9 X 4 S MacBook Air © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center I

Consider a buffer solution that consists of two separate components: the weak acid, CH3COOH(aq), and its conjugate base, CH3COO¯ (aq)  (added as NaCH3COO).   Which component will react with H+(aq) from a strong acid? Write the net ionic equation for the reaction that occurs when H+(aq) is added to the buffered solution.   Which component will react with OH-(aq) from a strong base? Write the net ionic                  equation for the reaction that occurs when OH-(aq) is added to the buffered solution.

By titration, it is found that 36.7 mL of 0.117 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.  I got 0.14862 - but is wrong.

An analytical chemist weighs out 0.275 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.0500M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 73.3 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g mol x10 X S

It is found that 41.27 ml of 0.2017 M NaOH is required to neutralize 25.00 ml of HNO3 solution in a titration experiment. Calculate the molarity of the HNO3 solution.

30)Which of the following reactions will not produce an ester? я А) B) б D) Е) F) CI OH SOH ОН OH + + CH₂N2 + OH OH OH OH HC1 HC1 H2SO4 NaOH

A solution of sodium cyanide, NaCN, has a pH of 11.90. How many grams of NaCN are in 615 mL of a solution with the same pH? Kb (CN–) = 1.7 × 10–5

Red cabbage juice is a sensitive acid-base indicator; its colors range from red at acidic pH to yellow in alkaline solutions. If red cabbage is used for the following titration, calculate the pH of the solution described and indicate whether the solution will be red or yellow.    If 67.00 mL of a 1.980 M HNO2 solution is reacted with 2.350 g NaOH, calculate the resulting pH.    Resulting pH = Color of Solution =

A chemistry graduate student is given 125.mL of a 0.40M ammonia NH3 solution. Ammonia is a weak base with Kb = 1.8x10−5. What mass of NH4Cl should the student dissolve in the NH3 solution to turn it into a buffer with pH = 9.03? You may assume that the volume of the solution doesn't change when then NH4Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.