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Find the pOH of a solution with: [H+] = 1.6×10-6 M pH = 5.80 ____________-

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Which two species act as bases in the acid-base reaction shown below? Select one: A. 1 and 2 B. 2 and 3 C. 1 and 3 D. 3 and 4 E. 2 and 4

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Formic acid, HCHO2, is used to make methyl formate (a fumigant for dried fruit) and ethyl formate (an artificial rum flavor). See the table for Ka.   What is the pH of a 0.21 M solution of formic acid?__________What is the degree of ionization of HCHO2 in this solution? __________

The hydronium ion concentration of an aqueous solution of 0.56 M phenol (a weak acid), C6H5OH, is [H3O+] = Submit Answer M References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining Podcasts LO 5 Previous Email Instructor Next Save and

Write the positive and negative ions that result when the following compounds are dissolved in aqueous solution: CaCl2 (aq) → Ca2+ (aq) + 2 Cl– (aq) Na2S (aq) ______________________________________________ (NH4)2CO3 (aq) ______________________________________________ K2SO4 (aq) ______________________________________________

If a sample of a certain solution is determined to have a [H3O+] concentration of 5.61 x 105 moles/liter, what is its pH? Round off your answer to one decimal place. Answer How to enter your answer (opens in new window) Keypad Keyboard Shortcuts

Part 1. Evaluate each statement and determine whether it is true or false Part 2. Classify the compounds as Arrhenius acid or Arrhenius base. Write N/A if it does not fit an of the classifications Part 3. Predict the products of the reaction of each pair of Arrhenius acid and Arrhenius base and write it's balanced equation

CHM 1360                                                      Lab 1 Buffers Worksheet Type your answers to the following questions. Make sure to use complete sentences. For images that need to be hand drawn, take a digital picture of your image and insert it into your worksheet. Insert your lab notebook image of the pH plot from your preparation of the acetate buffer.           Draw the Lewis structures for acetic acid (CH3COOH) and acetate (CH3COO-). On each structure, label the carboxylic acid or carboxylate functional group. Also, label the acidic hydrogen (if it has one).                In the first experiment you prepared a buffer by combining solutions of acetic acid and sodium acetate.   Write the chemical equation for the equilibrium of acetic acid and acetate in water. Include the states of the reactants.     Write a net ionic equation that shows how this buffer neutralizes added acid (HCl).      Write a net ionic equation that shows how this buffer neutralizes…

Which of the bases are strong bases and which are weak from Table 1? For the strong base,calculate the pH:

The pOH of a solution that has a pH equal to 5.31 is _________.     1.0 X 10-14     8.69     2.01 X 10-5     7.34 X 10-8

1. Nitrogen in an industrial wastewater is primarily in the form of ammonia (NH3) and ammonium (NH4+) ions. The acid/base equilibrium reaction for ammonia and ammonium is given as: NH4+ → H+ + NH3 Ką = 10-9.26 The total nitrogen concentration in wastewater is given as 2 x 10-3 moles/L (or 28 mg N/L), a. Calculate the concentration of ammonia (NH3) and ammonium (NH4*) ions at pH 10. NH3: moles/L NH4*: moles/L Check b. In ammonia stripping, nitrogen is removed from wastewater by volatilization of NH3. Would ammonia stripping be more effective above or below pH 9? Briefly explain your reasoning.

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a. Calculate the hydrogen ion concentration, in moles per liter, for a solution with a pOH of 4.60. M Concentration = b. Calculate the hydrogen ion concentration, in moles per liter, for a solution with a pOH of 7.34. Concentration = M c. Calculate the hydrogen ion concentration, in moles per liter, for a solution with a pOH of 12.76. Concentration = M

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You will work with a relatively dilute aqueous solution of hydrochloric acid in this week's lab. Let's review some of the hazards and cautions associated with HCI (aq). Identify if each of the statements below is TRUE or FALSE. HCI (aq) is corrosive - particularly at higher concentrations. When preparing a dilute solution of HCI, it is safest to slowly add concentrated acid to water. 1. TRUE HCI (aq) is flammable - even at low concentrations. 2. FALSE When preparing a dilute solution of HCI, it is safest to slowly add water to concentrated acid.

Acidic, Basic or Solution pH [OH] Neutral HCI (aq) 0.1 m 1x 10^-13 m acidic 1.0 H3BO (aq) 4.8 1.585 x 10^-5 m |1.58 x 10^-9 m acidic NHa (aq) 10.2 6.3 x 10^-11 m 1.58 x 10^-4 m basic NaOH (aq) 14 1x 10^-14 m 1m basic Solution [H') Acidic, Basic or pH [OH"] Neutral NazCOa (aq) 7.944 x 0.12 x 10^-4 m basic 9. 1.5^-10 m NaHCO: (aq) 8.5 3.6 x 10^-9 0.31 x 10^-5 basic NacI (aq) 7.3 5.01 x 10^-8 m 0.19 x 10^-6 basic NH CI (aq) 5.13 basic

The pOH of a solution 5.50 M is 5.50. What is its hydroxide-ion concentration? 3.2 x 10-5 M 3.2 x 10-6 M a. b. d. 3.2 x 10-7 M e. 3.2 x 10-9 M The pOH of a 0.015 M ammonia solution is 3.28. What is its hydroxide-ion concentration? C.