Question 24
1 Point
What is the pH of 1.94 x 10-5 M NaOH? (NaOH is a strong base) BLANK-1 (give your answer to 3 significant figures)
Question 24 1 Point What is the pH of 1.94 x 10-5 M NaOH? (NaOH is...
Question 23 1 Point What is the pH of 0.00187 M HCl? (HCl is a strong acid) BLANK-1 (give your answer to 3 significant figures) BLANK-1
Calculate the pH of a 7.5 x 10-5 M NaOH solution. Record your answer in the correct number of significant figures.
QUESTION 24 1 points Save Answer Calculate the pH at the equivalence point when 0.0100 M NaOH is used to titrate 0.0100 M chloroacetic acid, HC2H2C1O2. The Ka for chloroacetic acid is 1.4 x 10- 3 о Сансіо, нСанатоа оно 6.57 27.00 7.28 $1.43 " X = 7.14x10 0.0100 4*10-17 O 11.42 X= 7, 14x100 6.5X=2,67x107 Calculate the solubility at 25°C of CaF, in pure water and in a 0.0050 M NaF solution. You'll find Kindata in the ALEKS Data...
3. What volume of 0.025 M NaOH will be required to reach the endpoint in a titration with 25.00 ml of 0.10 M HCI? Show your work with units and correct significant figures. Circle your answer. 4. Calculate the molarity of a sodium hydroxide solution if 25.00 mL 0.100 M maleic acid requires 22.10 ml of NaOH to reach the endpoint. Show your work with units and correct significant figures. Circle your answer. 5. The following data were collected in...
QUESTION 2 The strong acid, HCl, is titrated with a strong base, NaOH, in aqueous solution. What is the pH of the titration solution after the addition of 17.94 mL of 0.100 M NaOH to a 50.00 mL of 0.100 M HCI? Write your answer using 3 significant figures,
24A) 40mL of 0.2 M formic acid is titrated with a strong base
(NaOH= 0.5 M). Determine the pH before any base has been added.
Please show steps and please explain why the answer is what it
is.
24B) The 40mL 0.2 M formic acid is titrated with a 6.0mL of
strong base. Here NaOH can be treated as a conjugate base and
formic acid is the acid.
please show steps and explain!
Us (24-25, Acid/base, aqueous equilibrium) 24A) (4...
PRE-LAB for plt.titeation.ofa 5tremsAcid.wth Bast This is due before the lab begins 1. Calculate the pH of the following solutions (a) 1 M NaC Name (b) I M HOAc (Ka-1.8 x 10-5) (c) I M NH4OH (Kb- 1.8 x 10-5) (d) 0.1 M NaOAc (e) 0.1 M NHCI 2 The pH of a 0.100 M solution of an acid, HA, is 1.70. Calculate the K? (use ICE) 2.Show your work with units and correct significant figures for all questions that...
Part B: A 30.0-mL volume
of 0.50 M CH3COOH (Ka=1.8×10?5) was titrated with 0.50 M NaOH.
Calculate the pH after addition of 30.0 mL of NaOH at 25 ?C.
Express the pH numerically.
MasteringChemistry: ASSIGNMENT #6 (Chapter 16)-Google Chrome https://session.masteringchemistry.com/myct/itemView?assignmentProblem ID=59386 148 CHEM 101 (M03) Help | Close NMENT #6 Titration of Weak Acid with Strong Base Resources Y previous | 19 of 25 | next » ± Titration of Weak Acid with Strong Base A certain weak acid, HA...
PRE-LAB for pH titration of a Strong Acid with Base This is due before the lab begins, Name 1. Calculate the pH of the following solutions: (a) 1 M NaCl Does not dissociate in water to produce either hydrogen or nyot thus it is a neutral Sall, so 7. (b) 1 M HOAc (Ka - 1.8 x 10-5) duce either hydrogen or hyd xde ion, (c) 1 M NHOH (Kb = 1.8 x 10-5) (d) 0.1 M NaOAC (e) 0.1...
Question 24 1 pts Calculate the pH of a 0.236 M solution of Sr(OH)2 Remember that a pH with three decimal places has three significant figures. Make sure to enter your answer with three decimal places. Question 25 1 pts Determine the pH at the equivalence point of a titration between 50.0 mL of 0.133 M (CH3)2NH solution with 0.133 MHCIO4. Remember that only the decimals in a pH count as significant figures. Please enter your answer with three decimal...