a) In the case of the addition of 0.3 moles of HOCl to 1 liter of solution, the concentrations of HCOl and OCl- are:
[HOCl] = 0.3 M
[OCl-] = 9.3x10 ^ -5 M
b) The concentration of HOCl in the equilibrium is practically the same, because the HCOl is a weak acid, this means that only a very small and negligible (for the calculations) part of the acid dissociates in the water and forms H3O + ions, but that small part makes a difference in pH of the solution.
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C) Add the missing values for HOCI] and (OCI-] to Table 2. Table 2. Characteristics of solutions ...
3) (ICE Analysis - 12 points) Consider a 1.0L aqueous solution at 298 K which is known to initially contain exactly 1.0 micromoles (1x10-6 moles) of the weak acid hypochlorous acid ( HOCI, PKA = 7.53) - i.e. this is what was added to the system initially before any chemistry or equilibration occurs. Assuming all activity coefficients are equal to 1.0, there are no others substances in the system, and that the only reaction that occurs in the system is:...
Name Formula К. Acetic acid CH3COOH 1.8 x 10-5 Formic acid HCOOH 3.0 x 10 Hydrazoic acid HN3 1.0 x 10-5 Hydrocyanic acid HCN 6.2 x 10-10 Hypochlorous acid HOCI 6.8 x 10-8 Nitrous acid HNOL 7.4 x 104 20. (7 pts) Use the table above to answer the following questions. A. Rank the following solutions in order from the lowest to highest pH. 0.10 M CH3COO- 0.10 M HCOO 0.10 M N 0.10 M OCI pH value: B. Write...
3.5 Exercise M -Relationship between concentrations, pH an Complete the following table for solutions at 259%C acidic, basic, neutral 2 8.32 1.00 4. 5.0x 10 1.0 x 10-12 Exercise J-Identifying acidic solutions by pH Circle the most acidic pH in each group: 2.5 1.5 10 2 12 0.9 1.5 1.3 7.4 12 7 10 5. 7.5 2.4 3.2 6. 8.5 3.8 11.2 7.6
A student following the procedure in this lab prepared 4 solutions by adding 12.00, 23.00, 26.00, and 34.00 mL of an 8.25 x 10-2 M NaOH solution to 50.00 mL of a 0.150 M solution of weak acid. The solutions were labeled 1, 2, 3, and 4 respectively. Each of the solutions was diluted to a total volume of 250 mL with DI water. The pH readings of these solutions were: (1) 6.38 (2) 6.73 (3) 6.80 (4) 6.98 PRE-LAB...
please show all work for part III :) all the information
needed is in the pictures
III. Preparing HC,HO, Solutions and Determining pH only cal. One! theoretical pH 1.0 x 10-14 (181) concentration of HC,H,O, M measured pH ya ? 3.06 1.0 x 10-2 ka: 1. 8x10°3 ixio- 3.43 1.0 x 10-3 x = CH) -1,34% 103n 3.87 1.0 x 107 PM - 04 TH11 4.30 concentration of HC,H,O, M calculated K of HC H302 based on pH data literature...
Preparing Buffer Solutions: Calculating the Volume of Weak Base Needed Use the table of K values given with this problem to choose the best weak base to start from for making a buffer that holds the pH of the solution at 5.00. Make your selection so that you maximize the capacity of the buffer. Assume that you want to make 700 mL of a buffer and you have already added enough of the conjugate acid salt to make the final...
Preparing Buffer Solutions: Calculating the Number of Grams of Conjugate Base Needed Use the table of K values given with this problem to choose the best weak acid to start from for making a buffer that holds the pH of the solution at 8.50. Make your selection so that you maximize the capacity of the buffer. Weak Acid K 1.8 X 10-5 6.5 X 10-5 1.5 X 10-5 You select a 800.0 ml volumetric flask to which you add 8.00...
Complete this table of values for four aqueous solutions at 25 "C HT] o] pH pOH Given Number Number Number 112.9 x 10-8 |M| | Solution A: Number Given Number Number Solution B: Number Number Given Number Solution C: In 4.97 Number Number Number Given Solution D: 11 □ 4.37 Given a diprotic acid, H2A, with two ionization constants of Kat = 1.5x10-4 and K2-4.4x10-11, calculate the pH for a 0.210 M solution of NaHA. Number Phosphoric acid, H3PO4(aq), is...
Preparing Buffer Solutions: Calculating the Volume of Weak Base Needed Use the table of K values given with this problem to choose the best weak base to start from for making a buffer that holds the pH of the solution at 9.70. Make your selection so that you maximize the capacity of the buffer. Assume that you want to make 100 mL of a buffer and you have already added enough of the conjugate acid salt to make the final...
values used for table 2
how do you do the Ice tables???
Experiment V. Equilibrium Constant Lab Report ( 50 pts) Calibration Curve 1. Record the absorbance for each of the standard solutions in the table below. Calculate the concentration of FeSCN)" in each of the standard solutions and record the values in the table below. Show a sample calculation (for A2) of your work in the space below the table. Solution Absorbance [Fe(SCN)" A-1 A-2 A-3 0.000 0.390 0.535...