Strong Acids; Calculate pH[HA]o[H;O"]pHStep 1Calculate [H3O] based on the fact that strong acids react completely with water.Step 2Calculate the pH using the equation:pH = -log (H;O"]What is the pH of a 1.73×10 M solution of the strong acid HC10,?HCIO,(aq) + H20(1) → C10, (aq) + H3o*(aq)[HC10], = 1.73×10-5Submit

given equation, HClO4(aq) + H2O(l)→ ClO4-(aq) + H3O+(aq) HClO4 is a strong acid with initial…

Answered: Strong Acids; Calculate pH [HA]o [H;O"]…

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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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
Using the constant below, calculate the molar concentration (M) of acid H3O* in solution if the concentration of OH- is 3.4 x 10-5. Kw = 1.0 × 10-14 M²= [H3O*][OH]. %3D O a) 2.9 x 10-10 O b) 2.0 x 10-10 O) 3,4 x 109 d) 2.4 x 10-10 e) 3.4 x 109
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
||| = O ACIDS AND BASES Determining the strength of acids from a sketch Four solutions of an acid dissolved in water are sketched below, as if under a microscope so powerful individual atoms could be seen. The same volume of solution is shown in each sketch. Note: Rank the solutions by the strength of the dissolved acid. That is, select 1 under the solution of the strongest acid, 2 under the solution of the next strongest acid, and so on. = H₂O Solution 1 (Choose one) Explanation Solution 3 (Choose one) Check ▼ ▬▬▬▬▬ Solution 2 (Choose one) ▼ Solution 4 (Choose one) 0/5 X spv7Aqws 3 Allie © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessi
Consider the following data on some weak acids and weak bases: acid base Ka Kb name formula name formula - 10 4.9 x 10 4 hydrocyanic acid HCN methylamine | CH3NH, | 4.4 x 10 C,H;NH2 4.3 × 10 HNO, 4.5 x 10 - 10 4 nitrous acid aniline Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' 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. solution pH 0.1 М КCN 4 (highest) 0.1 M C6H5NH3Br 1 (lowest) 0.1 M NaNO2 3 0.1 М KBr 2
Consider the following data on some weak acids and weak bases: acid base 9. name formula name formula HNO, 4.5 x 10 C;H;N |1.7× 10 nitrous acid pyridine hypochlorous acid 8. HСIО |3.0х 10 methylamine CH;NH, |4.4 × 10-4 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' 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. solution pH 0.1 М KCIO v choose one 1 (lowest) 0.1 M C5H5NHCI 3 0.1 M NaNO2 4 (highest) 3 0.1 М KNO3 choose one
The acid dissociation constant K, of hypobromous acid (HB1O) is 2.3 × 10 Calculate the pH of a 2.0 M solution of hypobromous acid. Round your answer to 1 decimal place. 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), 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
A solution is prepared that is initially 0.095 M in propanoic acid (HC2H5CO2) and 0.31 M in potassium propanoate (KC2H5CO2). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [H3O+]. You can ieave out the M/ symbol for molanty.
The equilibrium constant for an acid is called the acid ionization constant (Ka). If acetic acid (weak acid, HC2H3O2) is placed into water, it ionizes to H+ and C2H3O2- with a Ka of 1.82 x 10-5. Determine the pH of the solution when 20.0 g HC2H3O2 (s) is added to water, with a final volume of 1000. mL?
The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH - log [H+] where [H+] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 8.63 × 10-4 mol/L, the pH is == b. If the pH of a solution is 4.357, the hydrogen ion concentration is mol/L.
CH3CH2COOH Draw the Lewis structure of the acid and mark the acidic hydrogen with an asterisk (*). Draw a Lewis structure of the conjugate base of the acid. Suppose the acid is neutralized with a strong base. a) Which of the two structures you drew in 6 and 7 would be the predominant form of the species at a pH well above that at the equivalence point? b) Which of the two structures would be the predominant form of the species at a very low pH, well below that at the equivalence point and similar to the pH near the start of the titration? c) At what point in the titration, if any, would there be equal amounts of the two forms?

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