Strong Bases; Calculate pH[base][H3O"]pHStep 1The strong base dissociates completely in aqueous solution so [OH] = [base]. Use this to calculate the hydronium ion concentration.[H;O"][OH]= 1.0 x 10-14 at 25 °C.Step 2Calculate pH.pH = -log[H;O*]What is the pH of a 1.6x102 M solution of KOH at 25 °C?SubmitWhat is the hydronium ion concentration, [H30"], in the solution?|MSubmitBased on the hydronium ion concentration, what is the pH?[H;O*] = 6.3×10-13 MSubmit

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Answered: Strong Bases; Calculate pH [base]…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Use pH, POH, [H3O+], and [OH-] relationships. (a) The hydronium ion concentration in an aqueous solution of HCI is 7.2x10-2 M. Calculate [OH-], pH, and pOH for this solution. [OH-] = M pH = (b) The pH of an aqueous solution of KOH is 11.00. Calculate [H3O+], [OH-], and pOH for this solution. [H3O+] = M [OH-] = pOH = M pOH =
Consider the following data on some weak acids and weak bases: name hydrofluoric acid acid acetic acid solution 0.1MNHO 0.1 MC₂H₂Br 0.1 M Na 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. K 0.1 MKCH₂CD₂ formula HE 6.8x10 HCH,CO₂ 1.8x10 PH choose one choose one choose one choose one base S K₁ name formula ammonia NH, 1.8×105 pyridine C,H₂N 1.7×10
Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. Acidic Basic Neutral Answer Bank pH = 2.42 РОН %3D 5.35 РОН 3D 8.04 РОН %3D 7.00 [OH] = 8.8 x 10-3 pH = 8.11 [H+] = 9.9 × 10-2 [OH] = 3.2 x 10-9 %3D [H*] = = 1.0 × 10-7 H* = 5.9 × 10-12 %3D
The pH scale for acidity is defined by pH = - log1o H+] where H is the concentration of hydrogen ions measured in moles per liter (M). (A) The pH of ammonia is 11.0. Calculate the concentration of hydrogen ions in moles per liter (M). [H*] M (B) The pH of apples is 3.0. Calculate the concentration of hydrogen ions in moles per liter (M). [H*] = M
Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. Acidic pOH = 8.58 [H*] =3.4 x 10-2 pH = 8.24 [H+] = 5.4 x 10-12 pOH = 7.00 pH = 3.13 Basic Answer Bank [OH-] = 3.9 × 10-5 [OH-] = 1.3 x 10 Neutral [H]=1.0 x 10-7 pOH = 5.25
Strong Acids; Calculate pH [HA]o [H;O"] pH Step 1 Calculate [H30"] based on the fact that strong acids react completely with water. Step 2 Calculate the pH using the equation: pH = -log [H;O¯] What is the pH of a 1.73×10M solution of the strong acid HCIO,? HCIO,(aq) + H2O(t) → C10,(aq) + H30*(aq) [HCIO4]0 = 1.73×10-5 Submit What is the concentration of hydronium ion following reaction between the acid and water? Submit Calculate the pH of the solution based on the solution to the previous question (shown below). [H;O*] = 1.73x10-5 M
Two-Step Algebra a = -bc+d In order to solve the equation above for c, you must: Step One Add the same expression to each side of the equation to leave the term that includes the variable by itself on the right-hand side of the expression: |+a = -bc + d Submit
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.
Determine the pH of a solution with [H3o*] = 1.73 x 10-5 M. Your answer should contain 3 decimal places as this corresponds to 3 significant figures when dealing with logs. pH
A. What is the pH of an aqueous solution with a hydrogen ion concentration of [H*] = 8.1 x 10-5 M? pH B. What is the hydroxide ion concentration, [OH], in an aqueous solution with a hydrogen ion concentration of [H*] = 8.1 x 10-5 M? [OH-] = C. A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) = H*(aq) + A-(aq) The equilibrium concentrations of the reactants and products are [HA] = 0.190 M, [H*] = 4.00 x 104 M, and [A-] = 4.00 x 104 M. Calculate the Ką value for the acid HA. Ka = TOOLS x10"
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), 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 Bases LIOH, NaOH, КОН Strong Acids HCІ, HBr, HI HNO3 Ca(OH)2 (slightly soluble) HCIO4 Ba(OH)2 H2SO4 Sr(ОН)2
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 Question 1)What is the hydronium ion concentration in an aqueous hydrobromic acid solution that has a pOH of 10.200?[H3O+] = M

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