A solution has a $\mathrm{pH}$ of $4.5$. What would be the color of the solution if the following indicator was added?

methyl orange

A solution has a pH of 7.0. What would be the color of the solution if each of the following indicators were added? bromthymol blue

The active ingredient in aspirin is acetylsalicylic acid. A 2.51-g sample of acetylsalicylic acid required 27.36 mL of 0.5106 M NaOH for complete reaction. Addition of 15.44 mL of 0.4524 M HCl to the flask containing the aspirin and the sodium hydroxide produced a mixture with pH=3.48. Find the molar mass of acetylsalicylic acid and its $K _ { a }$ value. Acetylsalicylic acid is a monoprotic acid.

A solution has a pH of 7.0. What would be the color of the solution if each of the following indicators were added? thymol blue

Estimate the $\mathrm{pH}$ of a solution in which crystal violet is yellow and methyl orange is red.

Estimate the $\mathrm{pH}$ of a solution in which bromcresol green is blue and thymol blue is yellow.

Which of the indicators in the given figure earlier in the lessons could be used for doing the titrations below?

Titration of 25.0 mL of 0.100 M propanoic acid $\left(\mathrm{HC}_3 \mathrm{H}_5 \mathrm{O}_2\right.$, $K_{\mathrm{a}}=1.3 \times 10^{-5}$ ) with 0.100 M KOH.

Titration of 25.0 mL of 0.100 M pyridine $\left(K_{\mathrm{b}}=1.7 \times 10^{-9}\right)$ with 0.100 M hydrochloric acid.

Which of the indicators in the given figure earlier in the lessons could be used for doing the titrations below?

A 25.0-mL sample of 0.100 M lactic acid $\left(\mathrm{HC}_3 \mathrm{H}_5 \mathrm{O}_3, \mathrm{p} K_{\mathrm{a}}\right.$ $=3.86$) is titrated with 0.100 M NaOH solution.

Ttitration of 25.0 mL of 0.100 M propanoic acid $\left(\mathrm{HC}_3 \mathrm{H}_5 \mathrm{O}_2\right.$, $K_{\mathrm{a}}=1.3 \times 10^{-5}$ ) with 0.100 M KOH.

Which of the indicators in the given figure earlier in the lessons could be used for doing the titrations below?

Consider the titration of 80.0 mL of 0.100 M $\mathrm{Ba}(\mathrm{OH})_2$ with 0.400 M HCl.

Consider the titration of 100.0 mL of 0.100 M $\mathrm{H}_2 \mathrm{NNH}_2$ $\left(K_{\mathrm{b}}=3.0 \times 10^{-6}\right)$ with 0.200 M $\mathrm{HNO}_3$.

Which of the indicators in the given figure earlier in the lessons could be used for doing the following titrations?

Consider the titration of 40.0 mL of 0.200 M $\mathrm{HClO}_4$ with 0.100 M KOH.

Consider the titration of 100.0 mL of 0.200 M acetic acid $\left(K_{\mathrm{a}}=1.8 \times 10^{-5}\right)$ with 0.100 M KOH.

You have a solution of the weak acid HA and add some HCl to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how

A sample of a certain monoprotic weak acid was dissolved in water and titrated with 0.125 M NaOH, requiring 16.00 mL to reach the equivalence point. During the titration, the pH after adding 2.00 mL NaOH was 6.912. Calculate $K_{\mathrm{a}}$ for the weak acid.

A certain indicator HIn has a $\mathrm{p} K_{\mathrm{a}}$ of 3.00 and a color change becomes visible when 7.00% of the indicator has been converted to $\operatorname{In}^{-}.$ At what pH is this color change visible?

A student titrates an unknown weak acid HA to a palepink phenolphthalein endpoint with 25.0 mL of 0.100 M NaOH. The student then adds 13.0 mL of 0.100 M HCl. The pH of the resulting solution is 4.7. How is the value of $\mathrm { p } K _ { \mathrm { a } }$ for the unknown acid related to 4.7?