Enthalpy of Neutralization Notebook

Calculate final concentration

B. Molar Concentration of an Acid Solution Acid type, HA or H,A: HA Unknown No. Balanced equation for neutralization of acid with NaOH. NaOH + HCI = NaCI + Sample 1 Sample 2 Sample 3 1. Volume of acid solution (mL) 25.0 25.0 25.0 2. Buret reading of NaOH, initial (mL) 0.00 0.00 0.00 3. Buret reading of NaOH, final (mL) 26.3 26.0 26.8 26.3 26.0 0.148 4. Volume of NaOH dispensed (mL) 26.8 5. Molar concentration of NAOH (mol/L), Part A 6. Moles of NaOH dispensed (mol) 7. Molar concentration of acid solution (mol/L) 8. Average molar concentration of acid solution (mol/L) Data Analysis, B 9. Standard deviation of molar concentration Data Analysis, C 10. Relative standard deviation of molar concentration (%RSD) Data Analysis, D

"uonsanh stm The hydroxide ion concentration of an aqueous solution of 0.532 M acetylsalicylic acid (aspirin), HC9H¬O4, is [OH]= M. Submit Answer Retry Entire Group 9 more group attempts remaining Next 10/2 prt sc delete home fg ho 144 num & backspace %3D lock Y hc 3: 00 近

Given the following information complete the last (blank) data table

Volume vinegar used (mL)= 5.00 mL % from labe= l5 % Molarity of NaOH = 0.0976 M Titration volume measurements   Trial 1 Trial 2 Trial 3 Inital volume NaOH (mL) 0.69   0.86   0.16   Final volume NaOH (mL) 43.47   43.36   43.03   Volume NaOH used (mL)             Average volume NaOH used (mL) Average volume NaOH used (L) Moles NaOH used (from avg volume) Moles CH3COOH Molarity CH3COOH (mol/L) Mass CH3COOH (g) % (m/v) CH3COOH in vinegar

Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 2.29   1.41   1.95   Molarity of NaOH (M) 0.100   0.100   0.100   Volume of vinegar sample (mL) 5.00   5.00   5.00   Final burette reading (mL) 50.37   49.39   49.84 Table 2. Titration data   Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 2.29   1.41   1.95   Molarity of NaOH (M) 0.100   0.100   0.100   Volume of vinegar sample (mL) 5.00   5.00   5.00   Final burette reading (mL) 50.37   49.39   49.84   Expected color at end point       Volume of NaOH used (mL) 48.08   47.98   47.89  Compute for the ff: a.   Average moles of acetic acid (mol)? b.  Average molarity of acetic acid (M)? c.  Average molarity of acetic acid (M)?

MISSED THIS? Read Section 18.6 (Pages 823-826); Watch IWE 18.12. Determine the minimum concentration of the precipitating agent on the right to cause precipitation of the cation from the solution on the left. 9.0x10-2 M Cala; K2SO4 Express your answer using two significant figures. [K₂SO4]= ΜΕ ΑΣΦ Submit Request Answer Part C 1.7x103 M AgNO3; RbCl Express your answer using two significant figures. [RbCl] ΜΕ ΑΣΦ Submit Request Answer M M

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Table 2. Titration data   Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.19   2.26   2.39   Molarity of NaOH (M) 0.100   0.100   0.100   Volume of vinegar sample (mL) 5.00   5.00   5.00   Final burette reading (mL) 48.55   49.43   49.99   Expected color at end point             Volume of NaOH used (mL)           Average Volume of NaOH used in liters   Average moles of NaOH used (mol)   Average moles of acetic acid (mol)   Average molarity of acetic acid (M)     Average mass of acetic acid (g)   Average mass of vinegar (g) (assume the density of vinegar is 1.00 g/mL)   Average mass % of acetic acid in vinegar   Known mass % of acetic acid in vinegar is 5.45%   Percent Error

Molarity of NaOH Solution:   0.15 M NaOH   Trial 1 Trial 2 Trial 3 Mass of Unknown Acid 0.242 g 0.222 g 0.223 g Volume of NaOH soln. titrated 32.50 mL 31.2 mL 30.01 Moles of NaOH 0.004875 0.004875 0.004875 Moles of unknown acid       Calculated Molar mass of acid           Average Molar Mass of unknown acid

Why does it conduct more before and after this minimum point?

For question 5 could you find the best value and explain how you arrive to the best value please thank you!

2A student used a pipette to add 25 cm³ of sodium hydroxide of unknown concentration to a conical flask. The student carried out a titration to find out the volume of 0.1 mol/dm3 sulfuric acid needed to neutralise the sodium hydroxide. The following is the table of results obtained. Titration Volume of sulfuric acid used/cm³ 1 27.85 27.30 27.25 27.10 27.30 a. Write down a balanced equation for the reaction between sodium hydroxide and sulfuric acid. b. Describe the titration experimental procedure (details of washings are expected) c. Determine the average titre value and explain your choice of titre values in calculating the average. d. Determine the concentration of sodium hydroxide. e. If instead of sulfuric acid, hydrochloric acid of the same concentration was used what would you expect the average titre value to be and why?

1.10 M Acetic acid 0.900 M Sodium acetate [H30*1 (M) Solution (mL) |(mL) 1 8.00 2.00 8.71e-5M 2 7.00 3.00 5.13e-5M 6.00 4.00 3.24e-5M 4 5.00 5.00 2.17e-5 5 4.00 6.00 1.45e-5M 6. 3.00 7.00 9.31e-6M 7 2.00 8.00 1.00 9.00 00

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Trial 1: Initial pH= 3.92mL Mass of KHP and Paper= 0.868g Mass of paper= 0.357g Mass of KHP= 0.511g Trial 2: Initial pH= 4.09ml Mass of KHP and Paper= 0.870g Mass of paper= 0.359g Mass of KHP= 0.511g 1) find the volume at halfway point and the pH at halfway point of both trial 2) find the pKa of both trial and the mean pKa then use it to calculate Ka for KHP.

Hello! Could you please answer this with one long dimentional analysis like I am supposed to do it? Thank you!

Vinegar Ammonia Lemon juice Shampoo Detergent CC Hair Conditioner Mouthwash Antacid Aspirin Buffer Solutions H₂O 0.1 NaCl Solution A Solution B BY NC SA Color with pH Paper orange dark blue orange orange - green orange orange green-blue orange Initial pH 7.0 5.0 3.0 10.0 pH using pH Paper 2.0 13.0 3,0 3.0 6.0 4.0 4.0 10.0 pH after 5 Drops HCI 5.0 3.0 3,0 10.0 3.0 pH using pH Meter 3.0 2.67 11.11 2.76 3.0 10,0 4-58 Report Table AB.2: Effect of Adding Acid 8,60 4.62 4.58 8.64 3.11 pH after 10 Drops HC1 2.0 Acidic, Basic, or Neutral Total pH Change acidic Basic acidic acidic basic acidic acidic basic acid Buffer? (Y or N) Catalyst Education OER Labs are licensed under a Creative Commons Attribution-NonCommercial-ShareAlike 4.0 license. To access our full list of experiments visit https://links.labflow.com/OER. Lab Version AB Release 3.28. AB

14- 12- 10- PH 8. 6- 2- 0- 0 20.0 40.0 Volume of Titrant Added (mL) 60.0 80.0 A solution of 0.100 M HCI and a solution of 0.100 M NaOH are prepared. A 40.0 mL sample of one of the solutions is added to a beaker which is then titrated using the other solution. A pH electrode is used to obtain the data plotted in the titration curve shown here. a. Identify the solution that was initially added to the beaker. Explain your reasoning. b. On the titration curve, circle the point which corresponds to the equivalence point.

Determine the mean value of the solubility product for calcium iodate and the average deviation for your three trials.

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ist X b Answered: Thi x E # F3 X F4 $ Consider the X Chelp pleasel v X C Complete the balanced neutralization equation for the reaction below. Be sure to include the proper phases for all species within the reaction. KOH(aq) + H₂SO4(aq) → F5 % C 1 + F6 4 2 0₂ Reset S 3 F7 DOOG Question 2 of 21 & The pOH of a X 0² 0 4 5 04 s 5 H 8 = the ph of an a X ☐ ☐²+ ³+ 4+ 6 7 K Reaction Stoi X 8 9 0 6 7 8 ☐☐o (s) (1) (g) (aq) xH₂O O Delete PHSC + Insert Write the for X Delete Backspace +

Full solution pls

IA Cancel RESET Done A weak monoprotic acid HX is 1.5 % ionized in a 0.25 M solution of the acid. Determine the dissociation constant, Ka, of the acid. Answer: Use the format 1.2E-3 to report the number 1.2 x 10-3, for example. · $ Adjust Filters Crop | | |

10:57 H₂O 0.1 NaCl Solution A Solution B Initial pH 7.0 5.D 3.0 10.0 Acid-Base Titration % acidity from vinegar label Molarity of NaOH 2030 Volume of Vinegar (ml) Initial Volume of NaOH (ml) Final Volume of NaOH (mL) Report Table AB.3: Effect of Adding Base pH after 5 Drops NaOH 11.0 9.0 3.0 11.0 Acid/Base Titration, Buffers, and PH Report Sheet pH after 10 Drops NaOH 5% 0.101 Trial 1 Report Table AB.4: Concentration of Acetic Acid in Vinegar 11.0 12.0 3.0 11.0** 5.00 ML 0.00 ML 41.20 ML Total pH Change Trial 2 5,00 ML 000 ML 38.40mL Buffer? (Y or N) Trial 3 Show your calculations for calculating the %(m/v) for acetic acid in vinegar for Trial 1 in Report Table AB.4. X 5.00 ML 0.01 ML 41.30mL

How do you find the moles of NaOG needed to titrate KGP and the molarity of NaOH? I have some information listen but I so confused on how to get it with the information I have. The molarity might be 0.1 but like I said I don’t know if thats true or how you would get it. I’ve seen other people use it though.