Determine the pH of a solution that has a hydrogen ion concentration [H+] equal to 3.2x10-5 mol/L.

pHpH is a logarithmic scale used to indicate the hydrogen ion concentration, [H+], of a solution: pH=−log[H+] Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, [OH−], are related to each other by the Kw of water: Kw=[H+][OH−]=1.00×10^−14 where 1.00×10^−14 is the value at approximately 297 K. Based on this relation, the pH and pOH are also related to each other as 14.00=pH+pOH The temperature for each solution is carried out at approximately 297 K where Kw=1.00×10^−14 A. 0.20 g of hydrogen chloride (HCl) is dissolved in water to make 5.5 L of solution. What is the pH of the resulting hydrochloric acid solution? B. 0.20 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 3.0 L of solution. What is the pH of this solution? C. Calculate the concentration of HSO4− ions in a 0.010 M aqueous solution of sulfuric acid.

What are the concentrations of hydrogen ion and hydroxide ion in household ammonia, an aqueous solution of NH3 that has a pH of 11.50?  What is the concentration of hydroxide ion in household ammonia, an aqueous solution of NH3 that has a pH of 11.50?     M  OH-      What is the concentration of hydrogen ion in household ammonia, an aqueous solution of NH3 that has a pH of 11.50?     M  H+

4*) The autoionization constant for water at 35 °C is 2.2 × 10−14. Use this information to answer the following questions. a)What is the [H3O+] and pH of neutral water at 35 °C? b)Determine if the following solutions are acidic, neutral, or basic at 35 °C. Explain your answer. i)[H3O+] = 9.8 × 10−6 M ii)pH = 6.95 iii)[OH−] = 5.1 × 10−7 M iv)pOH = 9.24

Consider the following data on some weak acids and weak bases: name nitrous acid acid hypochlorous acid 0.1 M NaI solution 0.1 M KCIO 0.1 M C5H5NHBr 0.1 M NH4CI formula HNO₂ HCIO Ka 4.5 x 104 3.0 × 108 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. PH choose one choose one ✓ choose one base choose one name formula K₂ -5 ammonia NH3 1.8 × 10 pyridine CHN 1.7 × 10⁹

Determine the pH of a solution of a weak acid (HA) that is 0.0072 M. The Ka of the weak acid is 1.9 x 10-8

Which of the following statements is true?   a basic solution has an H3O+ concentration greater than 1.0 x 10-7 M and a pH value lower than 7.0.   a basic solution has an OH- concentration greater than 1.0 x 10-7 M and a pH value lower than 7.0.   a basic solution has an H3O+ concentration greater than 1.0 x 10-7 M and a pH value greater than 7.0.   a basic solution has an OH- concentration lower than 1.0 x 10-7 M and a pH value greater than 7.0.   a basic solution has an H3O+ concentration lower than 1.0 x 10-7 M and a pH value greater than 7.0.

Calculate the pH of the solution. Assume 5.0 L of solution. You must identify the type of solution before calculating the pH. Express all pH values to two decimal places. 0.190 moles NH3 and 0.120 moles HCl K(NH3) = 1.8 x 10-5

Determine the pH of a 7.98 × 10-3 M Ca(OH)2 solution.  Your answer should contain 3 decimal places as this corresponds to 3 significant figures when dealing with logs.    pH =

Strong acids and strong bases ionize 100% in aqueous solution.- HCl is a strong acid. In solution we write it as H+(aq) + Cl -(aq).- HF is a weak acid. In solution we write it as HF(aq).- KOH is a strong base. In solution we write it as K+(aq) + OH -(aq).- NH3 is a weak base. In solution we write it as NH3(aq).Exception: Since Ca(OH)2 is only slightly soluble we write it as Ca(OH)2(s).Below is a list of the 6 strong acids and 6 strong bases you should know. All other acids and bases are considered weak. Strong Acids Strong Bases HCl, HBr, HI LiOH, NaOH, KOH HNO3 Ca(OH)2 (slightly soluble) HClO4 Ba(OH)2 H2SO4 Sr(OH)2 What is the hydronium ion concentration in an aqueous hydrochloric acid solution with a pH of 4.250?[H3O+] =  M