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

phenolphthalein

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? crystal violet

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

One method for determining the purity of aspirin (empirical formula $\mathrm { C } _ { 9 } \mathrm { H } _ { 8 } \mathrm { O } _ { 4 } )$ is to hydrolyze it with NaOH solution and then to titrate the remaining NaOH. The reaction of aspirin with NaOH is as follows:

$$\begin{array} { l } { \mathrm { C } _ { 9 } \mathrm { H } _ { \mathrm { 8 } } \mathrm { O } _ { 4 } ( s ) + 2 \mathrm { OH } ^ { - } ( a q ) } \\ { \text { Aspirin } } \end{array} \frac { \text { Boil } } { 10 \mathrm { min } }\rightarrow \begin{array} { l } { \mathrm { C } - \mathrm { H } _ { 5 } \mathrm { O } _ { 3 } ( a q ) + } \\ { \text { Salicylate ion } } \end{array} \begin{array} { l } { \mathrm { C } _ { 2 } \mathrm { H } _ { 3 } \mathrm { O } _ { 2 } - ( a q ) + \mathrm { H } _ { 2 } \mathrm { O } ( l ) } \\ { \text { Acetate ion } } \end{array}$$

A sample of aspirin with a mass of 1.427 g was boiled in 50.00 mL of 0.500 M NaOH. After the solution was cooled, it took 31.92 mL of 0.289 M HCl to titrate the excess NaOH. Calculate the purity of the aspirin. What indicator should be used for this titration? Why?

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.