Solved: Are C2H5NH3Br, NaClO, NH4ClO, and KCl acidic or basic? How do you know? By signing up, you'll get thousands of step-by-step solutions to...

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Answer to: Use the Henderson?Hasselbalch equation to calculate the pH of each solution: a) a solution that is 0.115 M in HClO and 0.170 M in KClO...

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The pH of a solution of ethylamine, C2H5NH2 (Kb = 6.4 × 10-4) and ethylammium bromide, C2H5NH3Br is 11.00. What is the molarity of C2H5NH3Br if the molarity of C2H5NH2 is 0.025 M? Sorry ignore the typooo..please help

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Solution for Consider the following data on some weak acids and weak bases: acid Ka base name formula K, name formula nitrous acid HNO, 4.5 x 10* CH;NH, 4.3 x…

pH is a mathematical term which is equal to the –log of the H+ concentration of a solution (pH = –log[H+]. ... NH4Cl, CH3NH3NO3, and C2H5NH3Br are three examples ...

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39. Use the Henderson-Hasselbalch equation to calculate the pH of each solution. a. a solution that is 0.135 M in HClO and 0.155 M in KCIO b. a solution that contains 1.05% C2H5NH2 by mass and 1.10% C2H5NH3Br by mass c. a solution that contains 10.0 g of HC2H2O2 and 10.0 g of NaC,H,O, in 150.0 mL of solution

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The question goes: What is the pH of a 0.1 M solution of each of the following salts?Before you begin, estimate the pH (neutral, acidic or basic). a.MgF2 b.(NH4)2SO4 c.MgCl2 d.KCH3CO2 If someone c

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Jan 18, 2008 · low pH is acid. pH 7 is neutral. high pH is basic, (alkali) ( hydroxide present). You can test the pH of a solution by dipping pH paper into the solution and looking at the colour that is changes to. Red to yellow=acid. green=neutral. blue to purple=alkali

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What is the pH of a solution that is (a) Prepared by dissolving 3.30 g of (NH4)2SO4 in water, adding 125.0 mL of 0.1011 M NaOH, and diluting to 500.0 mL? (b) 0.120 M in piperidine and 0.010 M in its chloride salt?

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‹ pH = 14.00 ! pOH = 14.00 ! 2.30 = 11.70. 2 moles HCl reacts with 1 mole Ba(OH) 2 (or 2 moles OH!(aq)) For H+, ratio = (0.010 mol) ÷ 2 moles = 0.0050 For OH!, ratio = (0.020 mol) ÷ 2 moles = 0.010 ‹ OH!(aq) is in excess and H+ is the limiting reactant. pOH = ! log [OH!] ...

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Sep 23, 2016 · You prepare a 1L solution of 0.5 M imidazole. (pKa= 7.05). Calculate the pH of the solution after you add 0.1 moles of HCl. I need to create an ICE table. I also know I need to use the Henderson- Hasselbalch equation but I'm confused on what to plug in.