Question

Three solutions of Triblu indicator, all of equal concentration, were made at pH 1, pH 6...

Three solutions of Triblu indicator, all of equal concentration, were made at pH 1, pH 6 and pH 10. The pH 1 solution had an absorbance at 620 nm of 0.378, while the pH 10 solution had an absorbance of 0.545. If Triblu indicator has a pKa of 5.0, what would the absorbance of the pH 6 solution be at 620 nm? Answer to three decimal places.

Homework Answers

Answer #1

1. The universal indicator is not a single chemical compound,but a mixture of all the mentioned indicators. At pH it will begreen or greenish blue in color as indicated by the color in range6.2 to 7.6.

At pH 1.2 it will be red. Hence, option B is correct.

2. Since there is no indicator for the range of 7.6 to 8.0, theindicator will be unable to disti8distithis range. Option A iscorrect.

3. NaCl(s) Na+(aq) +Cl-(aq) Option A and B are correct.

4. CaCl2(s) Ca2+(aq) +2Cl-(aq) Option C and D are correct.

5. CH3COONa(aq) CH3COO-+ Na+ Option C and D are correct.

6. Na2CO3 2Na+ +CO3 2- Option A and B are correct.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Question 1 Calculate analytical concentration for each of the following solutions: a) HCl solution, pH =...
Question 1 Calculate analytical concentration for each of the following solutions: a) HCl solution, pH = 1.34 b) Acetic acid solution, pH = 4.31 c) Sulfuric acid solution, pH = 2.21 d) Potassium hydroxide solution, pH = 12.21 Acetic acid: pKa = 4.76 Sulfuric acid: pKa,1 = strong, pKa,2 = 1.99 In water, [H3O+][OH–] = 1.00 ! 10–14 Ignore the effect of ionic strength.
Please show all the work for the following pH calculations. What’s the pH if [H+] =...
Please show all the work for the following pH calculations. What’s the pH if [H+] = 10 mM? What’s the pH if [OH-] = 1 x 10-6 M? What’s the hydrogen ion concentration if pH = 4.76? What’s the hydrogen ion concentration if hydroxide concentration is 1 nM? What’s the pKa of a pH 6 solution with 0.075 M and 0.025 M respectively of HA and A-?
The Ka value for methyl red, a common pH indicator, is 5.0 x 10-6. HMR is...
The Ka value for methyl red, a common pH indicator, is 5.0 x 10-6. HMR is red, while MR- is yellow. What is the ratio of HMR to MR- and what color is a solution containing methyl red if the pH = 4.00?
1. The printed label on a bottle of commercial vinegar states that the acetic acid concentration...
1. The printed label on a bottle of commercial vinegar states that the acetic acid concentration is 5%. (Assume % is weight solute/volume solution) (a) If the manufacturer had reported two significant figures in the concentration, what range of values would round to 5.0 %? (b) Calculate the concentration in molarity of the upper and lower values from (a). The molecular weight of acetic acid is 60.05 g/mol. Pay attention to significant figures. 2. Acetic acid is a monoprotic weak...
Bromothymol blue is a chemical indicator that turns blue at a pH value greater than 7....
Bromothymol blue is a chemical indicator that turns blue at a pH value greater than 7. In which of these solutions would a colour be observed if 2 drops of cromothyml blue were added? The concentration of each solution is 0.10 M. Ka for HC2H3O2(aq) = 1.8 * 10^-5; Kb for NH3 (aq) = 1.8 * 10^-5 A - NH4Cl B - NaNO3 C - NH4C2H3O2 D - NaC2H3O2
Calculate the pH of each of the following strong acid solutions. 1. 20.00 mL of 1.50...
Calculate the pH of each of the following strong acid solutions. 1. 20.00 mL of 1.50 M  HCl diluted to 0.480 L . Express the pH of the solution to three decimal places. 2. A mixture formed by adding 46.0 mL of 2.5×10−2M  HCl to 120 mL of 1.5×10−2M  HI. Express the pH of the solution to two decimal places.
Determine the pH of each of the following solutions. Part A: 8.23×10−2 M HClO4 Express your...
Determine the pH of each of the following solutions. Part A: 8.23×10−2 M HClO4 Express your answer to three decimal places. Part B: A solution that is 4.8×10−2 M in HClO4 and 5.0×10−2 M in HCl Express your answer to two decimal places. Part C: A solution that is 1.04% HCl by mass (Assume a density of 1.01 g/mL for the solution.)   
QUESTION 1: What is the pH of an aqueous solution with a hydrogen ion concentration of...
QUESTION 1: What is the pH of an aqueous solution with a hydrogen ion concentration of [H ] = 5.6 × 10–5 M? QUESTION 2: Complete this table pf values for thre aqueous solutions at 25C. [H]+ [OH-] ph Solution A 7.7*10^-6 M X X Solution B X 0.097 X Solution C X X 8.84
A solution of equal concentrations of lactic acid and sodium lactate was found to have pH=3.85....
A solution of equal concentrations of lactic acid and sodium lactate was found to have pH=3.85. (a) What are the values of pKa, and Ka of lactic acid? (b) What would the pH be if the acid had twice the concentration of the salt? (c) Plot a graph showing a mole fraction of Lactic acid and Lactate with respect to pH. (You can use excel or any software of your choice). (d)There are many organic acids and bases in our...
question 3 Just as pH is the negative logarithm of [H3O+], pKa is the negative logarithm...
question 3 Just as pH is the negative logarithm of [H3O+], pKa is the negative logarithm of Ka, pKa=−logKa The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions: pH=pKa+log[base][acid] Notice that the pH of a buffer has a value close to the pKa of the acid, differing only by the logarithm of the concentration ratio [base]/[acid]. The Henderson-Hasselbalch equation in terms of pOH and pKb is similar. pOH=pKb+log[acid][base] Part A Acetic acid has a Ka of 1.8×10−5....
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT