The concentration of a solution is measured with a potentiometer called a pH meter. O H* O H20 OH CH3CO" + O Na*

What are the equilibrium concentrations of NH3, NH4+, and OH in a 0.78 M solution of ammonia? Kb = = 1.8 × 10-5 [OH-] [NH₂+] = [NH3] = What is the pH of the solution? pH = M M M

||| ctrl lacc shift ↑ tab caps lock VILION Mc ALE Graw HI esc K →1 Pavilion x360 fn O CHEMICAL REACTIONS Determining the molar mass of an acid by titration McCA X Eplanation g mol V An analytical chemist weighs out 0.188 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1500M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 38.4 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. f1 Type here to search A https://www-awu.aleks.com/alekscgi/x/Isl.exe/1o_u-IgNslkr7j8P3jH-IvUrTNdLZh5A8CnG03PBGuXr8iCPa7ZMmym f2 @ Z Check 2 L M W hp S ALE MCCA ALER f3 # Mc Graw 3 X alt D 4 $ 4 с x10 X R O f5 Me Graw MI % F 5 at 40 MCCA ALE ALE ● V T S f6 4- G 6 ■ T f7 B Y ♫+ & Mc 7 H raw fg MCCA ALER *. N KAA © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center |…

Consider the “window cleaner” problem, question 2 on page 12 of your lecture notes. Suppose that prior to the titration, the 10 mL sample of window cleaner was diluted by adding about 10 mL of DI water so that the solution could have better contact with the pH meter. What effect would this dilution have on the volume of titrant needed? (a) The amount of titrant would be the same because the moles of analyte was not changed.(b) The amount of titrant would be doubled because the analyte solution volume was doubled.(c) The amount of titrant would be halved because the was diluted by half.

it pt Calculate the pH of a solution that has an ammonium chloride concentration of 0.042 M and an ammonia concentration of 0.047 M. pH = Ky=1.8 x 10-

Calculate the molarity of an NaOH solution from the following titration data.  Be sure the answer has the correct amount of significant figures.  The chemical equation for this titration is as follows: NaOH  +  KHP  ⟶  NaKP  +  H2O NaOH buret reading, inital:  15.27 mL NaOH buret reading, final:     8.32 mL Mass of KHP (204.22 g/mol):  1.1592 g Calculate the molarity of an NaOH solution from the following titration data.  Be sure the answer has the correct amount of significant figures.  The chemical equation for this titration is as follows: NaOH  +  KHP  ⟶  NaKP  +  H2O NaOH buret reading, inital:  15.27 mL NaOH buret reading, final:     8.32 mL Mass of KHP (204.22 g/mol):  1.1592 g

the solution has to be acidified before testing for Ag+ ions. To make sure that the solution is acidic, what should be done?     Apply a drop of the solution to red litmus paper to see if it turns blue.     Apply a drop of the solution to blue litmus paper to see if it turns red.     Apply a drop of the solution to pH paper to see if the pH is above 7.     Apply a drop of the solution to your tongue to see if it tastes sour.

a Calculate the molar concentration of OH in a solution that contains 8.7×10-¹2 M H30+. (Enter your answer to two significant figures.) [OH-] = M bCalculate the molar concentration of OH in a solution that contains 3.5×10-3 M H30+. (Enter your answer to two significant figures.) [OH-] = M

What is the concentration of H* in 0.042 M HCIO4? [H*] = i What is the pH of the solution? pH = M What is the OH- concentration in the solution? For scientific notations, use the format 1.0E-10, for example. [OH-] = i M By how much does the pH change if the concentration of H* is doubled? i

Please answer all parts.