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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? __________

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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) ______________________________________________

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Solve and show solution 1. What is the pH and pOH of a solution prepared by dissolving 10 g of Ba (OH)2 in water to make a 1 L solution? 2. Determine the hydrogen/hydroxide ion concentration of the solution given the following pH below. a. pH=2.4 b. pH= 8.5 Answer question 1 and 2 a and b. Thank you

________________ are substances that react with, or accept, H+ ions; they increase the concentration of OH– when dissolved in water.

PLEASE PLACE THE ANSWERS IN A SQUARE BOXES SAME AS THE QUESTION. SO I COULD KNOW WHICH ANSWERS BELONGS TO THE RIGHT PLACE.

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

Calculate the hydronium ion concentration, [H3O+], for a solution with a pH of 6.73.   [H3O+]=___________M

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…

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An aqueous solution contains 0.417 M nitrous acid. Calculate the pH of the solution after the addition of 5.38x10-2 moles of sodium hydroxide to 250 mL of this solution. (Assume that the volume does not change upon adding sodium hydroxide). pH = *3 # Submit Answer 80 E C $ 4 R F Retry Entire Group 5 more group attempts remaining % Use the References to access important values if needed for this question. 5 V Cengage Learning | Cengage Technical Support T G 6 B Y H & 7 U N * 8 J A I M ( 9 K 7 O < ) 0 1 4 P ^. Previous Email Instructor Save and Exit + 11 { [ O Next = L de

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

A) What is the pH of a 5.58×10-5 M solution of the strong acid HCl? HCl(aq) + H2O(ℓ) → Cl-(aq) + H3O+(aq)[HCl]0 = 5.58×10-5 ____________________ B) What is the pH of a 4.4×10-2 M solution of KOH at 25 °C? ________________