{"id":30944,"date":"2025-06-21T20:55:23","date_gmt":"2025-06-21T20:55:23","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=30944"},"modified":"2025-06-21T20:55:24","modified_gmt":"2025-06-21T20:55:24","slug":"the-ph-of-an-aqueous-solution-of-0-226-m-ammonium-bromide-nh4br-aq-is-__","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/the-ph-of-an-aqueous-solution-of-0-226-m-ammonium-bromide-nh4br-aq-is-__\/","title":{"rendered":"The pH of an aqueous solution of 0.226 M ammonium bromide, NH4Br (aq), is __."},"content":{"rendered":"\n

The pH of an aqueous solution of 0.226 M ammonium bromide, NH4Br (aq), is __<\/strong><\/em><\/strong>. This solution is (ACIDIC\/BASIC\/NEUTRAL).<\/p>\n\n\n\n

The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n

Correct Answer:<\/strong><\/p>\n\n\n\n

The pH of a 0.226 M solution of ammonium bromide (NH\u2084Br) is approximately 4.82<\/strong>. This solution is acidic<\/strong>.<\/p>\n\n\n\n

\n\n\n\n

Explanation:<\/strong><\/p>\n\n\n\n

Ammonium bromide (NH\u2084Br) is a salt<\/strong> that forms when a weak base<\/strong> (ammonia, NH\u2083) reacts with a strong acid<\/strong> (hydrobromic acid, HBr). When this salt dissolves in water, it dissociates completely into its ions:NH\u2084Br (aq)\u2192NH\u2084\u207a (aq)+Br\u207b (aq)\\text{NH\u2084Br (aq)} \\rightarrow \\text{NH\u2084\u207a (aq)} + \\text{Br\u207b (aq)}NH\u2084Br (aq)\u2192NH\u2084\u207a (aq)+Br\u207b (aq)<\/p>\n\n\n\n

    \n
  • Br\u207b<\/strong> is the conjugate base of the strong acid HBr. It does not<\/strong> hydrolyze in water and has no effect on pH.<\/li>\n\n\n\n
  • NH\u2084\u207a<\/strong> is the conjugate acid of the weak base NH\u2083. It does<\/strong> hydrolyze in water, releasing H\u207a ions:<\/li>\n<\/ul>\n\n\n\n

    NH\u2084\u207a + H\u2082O\u21ccNH\u2083 + H\u2083O\u207a\\text{NH\u2084\u207a + H\u2082O} \\rightleftharpoons \\text{NH\u2083 + H\u2083O\u207a}NH\u2084\u207a + H\u2082O\u21ccNH\u2083 + H\u2083O\u207a<\/p>\n\n\n\n

    This reaction increases<\/strong> the concentration of hydrogen ions in the solution, making the solution acidic<\/strong>.<\/p>\n\n\n\n

    To calculate the pH, we use the Ka<\/strong> of ammonium ion. First, find Kb<\/strong> for NH\u2083:Kb (NH\u2083)=1.8\u00d710\u22125\\text{Kb (NH\u2083)} = 1.8 \\times 10^{-5}Kb (NH\u2083)=1.8\u00d710\u22125<\/p>\n\n\n\n

    Then use the relationship between Ka and Kb:Ka=KwKb=1.0\u00d710\u2212141.8\u00d710\u22125\u22485.56\u00d710\u221210K_a = \\frac{K_w}{K_b} = \\frac{1.0 \\times 10^{-14}}{1.8 \\times 10^{-5}} \\approx 5.56 \\times 10^{-10}Ka\u200b=Kb\u200bKw\u200b\u200b=1.8\u00d710\u221251.0\u00d710\u221214\u200b\u22485.56\u00d710\u221210<\/p>\n\n\n\n

    Now use the Ka expression to solve for [H\u2083O\u207a]:Ka=x20.226\u2192x2=(5.56\u00d710\u221210)(0.226)K_a = \\frac{x^2}{0.226} \\rightarrow x^2 = (5.56 \\times 10^{-10})(0.226)Ka\u200b=0.226×2\u200b\u2192x2=(5.56\u00d710\u221210)(0.226)x=1.26\u00d710\u221210\u22481.12\u00d710\u22125 Mx = \\sqrt{1.26 \\times 10^{-10}} \\approx 1.12 \\times 10^{-5} \\text{ M}x=1.26\u00d710\u221210\u200b\u22481.12\u00d710\u22125 M<\/p>\n\n\n\n

    Now calculate pH:pH=\u2212log\u2061[H3O+]=\u2212log\u2061(1.12\u00d710\u22125)\u22484.82\\text{pH} = -\\log[H\u2083O\u207a] = -\\log(1.12 \\times 10^{-5}) \\approx 4.82pH=\u2212log[H3\u200bO+]=\u2212log(1.12\u00d710\u22125)\u22484.82<\/p>\n\n\n\n

    Because the pH is less than 7, the solution is acidic<\/strong>.<\/p>\n\n\n\n

    \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

    The pH of an aqueous solution of 0.226 M ammonium bromide, NH4Br (aq), is __. This solution is (ACIDIC\/BASIC\/NEUTRAL). The Correct Answer and Explanation is: Correct Answer: The pH of a 0.226 M solution of ammonium bromide (NH\u2084Br) is approximately 4.82. This solution is acidic. Explanation: Ammonium bromide (NH\u2084Br) is a salt that forms when […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[],"class_list":["post-30944","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/30944","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/comments?post=30944"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/30944\/revisions"}],"predecessor-version":[{"id":30950,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/30944\/revisions\/30950"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=30944"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=30944"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=30944"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}