A chemist dissolves 134. mg of pure sodium hydroxide in enough water to make up 170. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Be sure your answer has the correct number of significant digits. 0 0x10 X

Use the formula pH=-log[H^+]. The variable pH represents the level of acidity or alkalinity of a liquid on the pH scale, and [H^+] is the concentration of hydrogen ions in the solution. Determine the value of [H^+] (in mol/L) for the following liquids, given their pH values. Express your answers in scientific notation with three significant digits.  a.) Tea pH=5.5  b.) Milk pH=6.2   What is the concentration of hydrogen ions in tea? What is the concentration of hydrogen ions in milk?

A solution of HA, a weak acid (pKa = 8.112), has a pH=5.770. [HA]eq = 3.12 x 104 M. What was the initial concentration of the weak acid soll the correct number of significant figures, into the box below. If your answer is a decimal, put a O before the decimal point. Do not use scientific notation. [weak acid] initially = pH = X X An aqueous solution of 0.045 M HA (pKa = 11.11) is prepared. What is the pH of this solution? Enter your answer, rounded to the correct number of significant figures, into the box below. If your answer is a decimal, put a 0 before the decimal point. Do not use scientific notation. 4.00 0.00404 M ***** MONTEXT MENT

Find the hydrogen ion concentration of a saturated solution of calcium hydroxide whose pH is 13.3. (If you enter your answer in scientific notation, round the decimal value to one decimal place. Use equivalent rounding if you do not enter your answer in scientific notation.)

Convert the following pH or pOH values to [H*] or [OH] concentration Example: pH = 7.0, [H*] = 1.0 x 10-7 M pH = 5.3, [H*] = РОН 3 11.1, [Н']]- РОН 3 6.6, [ОН]- pH = 2.5, [OH]] = In two or three sentences, compare and contrast the Bronsted-Lowry definition of acids/bases and the Arrhenius definition. What are the similarities and differences? Complete the acid-base equation, providing the missing species. Under each species, write A, B, CA, or CB for acid, base, conjugate acid, or conjugate base, respectively. H2O + HCO3 + H3O*

An aqueous solution at 25 °C has a H,O* concentration of 6.x 107 M. Calculate the OH concentration. Be sure your answer has 1 significant digits. Ом M ☐ x10 ×

Please fill out the pH table. Thanks!

Boiling water has a pH of 6.1. Does this mean that boiling water is acidic?      Explain your answer.

A chemistry student weighs out 0.0812 g of sulfurous acid (H₂SO3), a diprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1500M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Round your answer to 3 significant digits. mL x10 X S Elld ? ol Ar

Calculating molarity using solute mass A chemist prepares a solution of sodium nitrate (NaNO3) by measuring out 95.5 g of sodium nitrate into a 250. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's sodium nitrate solution. Round your answer to 3 significant digits. mol/L x10 1/3 Ś Olivia V ? 00 A