How do I do this without being give Kb or Ka? Please walk me through the...
In the titration of a 25 mL of 0.245 M weak base (Kb = 1.76*10^-5) being titrated by 0.365 M HCl determine the following: a. The PH at the initial point b. The PH after 12.3 mL of HCl has been added c. The PH at the equivalence point d. The PH after 18.4 mL of HCl has been added
correct answer is highlighted in pink. how do i get
the pH without it being 1.6?
Equilibrium Constants The following equilibrium constants will be useful for some of the problems. Substance H2CO3 Substance HCOH HNO2 НОСІ (COOH)2 Constant K = 1.8 x 10-4 Ka = 4.5 x 10-4 KA = 3.5 x 10-8 K = 7.2 x 10-4 KA = 4.0 x 10-10 Ki = very large K = 1.2 x 10-2 Ka=2.5 x 10-9 Constant Ki = 4.2 x...
please include how you solved for the answer
Calculate the pH at each of the following points along the titration of 20.0 mL of 0.17 M Ethylammine with 0.17 M HCl. [Kb = 2.3x10-) PK9 = 5.6 5.6 rog (17/17) -- 5.6 t5ml 5.6 x L x sm 1000 0 mL of HCI added pH = 5 mL of HCI added pH = 10 mL of HCI added pH = 15 mL of HCI added pH = 20 mL of...
I need help with #3, 4. Also, I am confused with #5
because both pH are the same.
Ka 1-7X10 4 3. In a titration between HCHO, and KOH, would the pH at the equivalence point be acidic, basic, or neutral? Briefly explain your answer. HCHO+KOH b) Which of the following acid-base indicators would be the best one to use in the titration? i) methyl orange, Ka = 104 ii) bromthymol blue, Ka = 10-7 iii) thymolphthalein, Ka= 10-10 4....
please help walk me through how to solve these, the questions
change everytime. i am not even sure where to start. thank
you
HON WILL UNULNEM TULENERAL CHEMISTRY LABE Amber Gloria's Qula History Lab & Quiz Exploring Buffers Background Incorrect Question 3 0/1 pts If you mix a weak acid and a weak base together with concentrations of 0.33 and the acid has apk, -8.58, what is the pH of the buffer? Give your answer to two decimals. pH =...
I
can't figure out how to find the concentration of the conjugate
base.
Question 2 If a 50.00 mL sample of 0.132 M ammonium chloride is titrated with 21.47 mL of 0.149 M NaOH, what is the pH of the titration mixture? (For NH4CI, Ka = 5.75 x 10-10, Selected Answer: 2 Correct Answer: 9.21 +0.02 Response This is in the buffered region of the titration. Therefore, calculate the moles of weak acid initially present and the Feedback: moles of...
Can someone please explain to me in detail how to do this problem? Please show all of the work and do not skip any steps! What is the pH at the equivalence point in the titration of 10.0 mL of 0.35 M unknown acid HZ with 0.200 M NaOH? Ka = 2.4x10-7 for the unknown acid HZ A] 7.00 B] 10.1 C] 4.14 D] 9.86
I am having trouble understanding this problem. Can you please
walk me through the steps using the BCA and ICE tables?
Calculate the pH of each of the solutions and the change in pH to 0.01 pH units caused by adding 10.0 mL of 3.68-M HCl to 300. mL of each of the following solutions Change is defined as final minus initial, so if the pH drops upon mixing the change is negative a) water pH before mixing7.00 pH after...
Find the pH at the equivalence point of HA being titrated by BOH, where HA is a weak acid with a ka=4.3*10-4 and BOH is a strong base you have Building on problem 1, if you have 0.1 M NaOH and find your equivalence point at 23.78 mL added, how many moles of HA were present? Find the equivalence point and the pH at equivalence of .234 moles of citric acid being titrated with 0.100 M KOH. Acetic acid is...
If you could please help me with these that would be
amazing! Thanks in advance
Pre-Lab Assignment for Experiment 19:Titration Curves Introduction: This pre-lab assignment will illustrate some of the important features of titration curves and what information can be obtained from them. A titration curve is the plot of the pH of a solution such as an acid or a base as a titrant is being added to it. A titrant is the solution being added from a buret,...