General Chemistry
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A solution of equal volumes of 0.50 M HCl and 0.30 M HNO3 was prepared. Find its pH. Note: Assume that volumes are additive.
How many grams of HNO3 are required to dissolve in 0.35 L of solution to obtain a pH of 1.95?
0.200 M KOH is used to titrate 50.0 mL samples of 0.200 M HNO3 and 0.200 M HNO2, individually. Match them to their corresponding titration curve.
Determine the pH and identify the main source of H3O+ in a 1.2 × 10-9 M solution of HCl. Also, determine the pH of 1.2 × 10-7 M HCl. (Hint: pH should not exceed 7.)
A solution containing 0.150 M HCl and 0.200 M HF is titrated with 0.150 M NaOH. Determine the initial pH of the solution before the addition of NaOH.
Which is the most basic solution?
The mixture of 0.14 M HCl and 0.19 M HF has a pH of _.
Calculate the pH of a 2.31% by mass solution of NaOH. The density of the solution is 1.02 g/mL.
Calculate the pH of a solution made by dissolving 150 mL of HI(g) (at 0.95 atm and 25 ºC) to make a 1.7 L aqueous solution.
Calculate pH, [H3O+], and [OH–] for a solution that is 0.026 M HCl and 0.018 M HBr.
For a 0.36 M HI solution, calculate pH, pOH, [H3O+], and [OH–].
A solution was prepared by dissolving 0.845 g barium oxide (BaO) in 150.0 mL water. What is the pH of this solution?
If 150.0 mL of 2.5×10–3 M HBr is mixed with 50.0 mL of 1.5×10–3 M HNO3, what is the pH of the resulting solution? Assume the volumes are additive.
An aqueous solution contains 1.45 g KOH in 455 mL. What is the pH of the solution?
Calculate the mass of lithium oxide (Li2O) required to be dissolved in 1.55 L of water to prepare a solution with a pH of 11.50.
Calculate the pH of a 2.64 × 10–3 M solution of Mg(OH)2 at 25 ºC.
Ba(OH)2 is an important laboratory reagent used for titrations. Calculate the concentration of an aqueous Ba(OH)2 solution having a pH of 9.850.
Calculate the [OH−] ion concentration and pH of a solution made by diluting 15.0 mL of 0.0225 M NaOH solution to a final volume of 545 mL.
What is the pH of a solution of 0.455 g HIO4 in 785 mL water?
What is the pH of a solution of 2.25 g HBr in 575 mL water?
A solution is prepared by dissolving 1.15 g of calcium oxide (CaO) in 2.25 L of water. What is the pH of the solution?
The pH of a colorless solution was measured using a pH meter as shown below. Is this a solution of HBr(aq) or a solution of NaOH(aq)? What is the molarity of the solution if the liquid is one of the solutions?
What are the pOH, pH, [H3O+], and [OH-] of a 1.2x10-3 M Sr(OH)2 strong base solution?
What is the pH, [H3O+], and [OH-] for a 0.732 % HClO4 by mass of a strong acid solution with a density of 1.02 g/mL?
Calculate the mass of HNO3 needed to prepare a 0.75 L of solution with a pH of 1.28.
What are the [OH-], [H3O+], pH, and pOH for 0.30 M KOH?
Calculate the [H+] of 3.4x10-5 M Ba(OH)2 solution.
Hydrochloric acid (HCl) is a commonly used laboratory reagent. It is a strong acid that dissociates completely in an aqueous solution into H+ and Cl−. If a 355 mL solution has a pH of 2.850, how many moles of H+ ions does the solution contain? How many grams of sodium hydroxide (NaOH) are required to completely neutralize the solution?
Acid rain is a serious environmental problem that damages the ecosystem, destroys materials, and has negative effects on human health. A limestone-made (CaCO3) Buddha statue in India has endured damage caused by acid rain. If 1.546×107 L of rainwater with a pH of 4.500 completely reacts with the statues, what mass of the statue (in kg) is lost?
Laboratory preparation of carbon dioxide (CO2) gas is often carried out by reacting limestone (CaCO3) with hydrochloric acid (HCl). The limestone dissolves completely into the acid solution and produces CaCl2, H2O, and CO2. Determine the volume (in mL) of a pH 1.100 HCl solution that could dissolve a 1.15 g piece of limestone. Could the same piece of limestone neutralize a 350 mL sample of HCl solution with a pH of 1.100? If not, what fraction can it neutralize?