Calculating the composition of a buffer of a given pH -5 A chemistry graduate student is given 500. mL of a 0.60M ammonia (NH3) solution. Ammonia is a weak base with K₁ = 1.8 × 10¯¯ should the student dissolve in the NH3 solution to turn it into a buffer with pH = 9.27? What mass of NH Br 4 You may assume that the volume of the solution doesn't change when the NHBr is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ☐ x10 ☑ ? 00. 18 Ar B

What quantity in moles of CH₃NH₃Cl  need to be added to 200.0 mL of a 0.500 M solution of CH₃NH₂ (Kb for CH₃NH₂ is 4.4 × 10⁻⁴) to make a buffer with a pH of 10.90?

A chemistry graduate student is given 250. mL of a 0.10M methylamine (CH3NH2) solution. Methylamine is a weak base with K 4.4 x 10 CH3NH2Br should the student dissolve in the CH3NH2 solution to turn it into a buffer with pH = 10.21? What mass of You may assume that the volume of the solution doesn't change when the CH3NH3Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0 ☐ x10 X G

A chemistry graduate student is given 125. mL of a 0.90M benzoic acid (HC,H,CO2) solution. Benzoic acid is a weak acid with K,=6.3 × 10 °. - 5 What mass of NaC,H,CO, should the student dissolve in the HC,H,CO, solution to turn it into a buffer with pH = 3.97? You may assume that the volume of the solution doesn't change when the NaCH,CO, is dissolved in it. Be sure your answer has a unit symbol, and round it 2. to 2 significant digits. x10

A chemistry graduate student is given 125. mL of a 1.30M dimethylamine ((CH,) NH solution. Dimethylamine is a weak base with K,=5.4 × 10 . What mass of (CH,), NH, Cl should the student dissolve in the (CH,) NH solution to turn it into a buffer with pH =10.80? You may assume that the volume of the solution doesn't change when the (CH, NH, Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 10

A chemistry graduate student is given 500.mL of a 0.80M chloroacetic acid (HCH2ClCO2) solution. Chloroacetic acid is a weak acid with Ka = 1.3x10^−3. What mass of NaCH2ClCO2 should the student dissolve in the HCH2ClCO2 solution to turn it into a buffer with pH = 3.08 ?You may assume that the  volume of the solution doesn't change when the NaCH2ClCO2  is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.

If you wanted to create a buffer with a pH = 3.2, what substances would you choose to make the buffer? Weak Acid K, pK, HCIO, 7.2 x 10-3 1.94 HNO, CH,COOH H,CO, 4.0 x 10-4 3.39 1.8 x 10-5 4.75 6.3 x 10-8 6,35 HBRO 2.8 x 10-9 8.55 HCO, 4.0 x 10-13 10.33 HNO, and NO, CH;COOH only HNO, only HCO; and CO,2 HBГО and BrO HCIO, and CIO, CH3COOH and CH;COO

We have to make a borate buffer with pH = 8.8 where the boric acid pKa = 9.00. If we start with a 1 liter of 0.1 M boric acid solution, what mass of hydroxide ions should be added to get the desired pH? Boric acid has the molecular formula B (OH) 3 and the borate ion B (OH)

A chemistry graduate student is given 500. mL of a 1.60M chloroacetic acid (HCH2CICO2) solution. Chloroacetic acid is a weak acid with K = 1.3 × 103. What mass of NaCH2CICO₂ should the student dissolve in the HCH2CICO2 solution to turn it into a buffer with pH =2.37? You may assume that the volume of the solution doesn't change when the NaCH2CICO2 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. Explanation Check G MacBook Air 2024 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility

A buffer is made using 100.0 mL of 0.100 M CH3CH2COOH (propanoic acid) and 100.0 mL of 0.100 M NaCH3CH2COO (sodium propanoate). 10.0 mL of 0.100 M HCl is added to the buffer. What is the solution pH after the HCl is added?For CH3CH2COOH K = 1.3 x 10^-5