Write reaction showing how each of the bufferswould neutralize added NaOH.HCHO2 and NaCHO2Express your answer as a balanced chemical equation. Identify all of the phases in your answer.0ΑΣΦSubmitA chemical reaction does not occur for this question.?Request Answer Part BWhat is the [H3O+]?Express your answer using one significant figure.[H3O+] =Submit15| ΑΣΦRequest Answer?M

A buffer is a solution which resist any change in pH on adding a small amount of acid or base . it…

Write reaction showing how each of the buffers would neutralize added NaOH. HCHO2 and NaCHO2 Express your answer as a balanced chemical equation. Identify all of the phases in your answer. ΑΣΦ ? A chemical reaction does not occur for this question. Submit Request Answer

Write reaction showing how each of the buffers would neutralize added NaOH. HCHO2 and NaCHO2 Express your answer as a balanced chemical equation. Identify all of the phases in your answer. ΑΣΦ ? A chemical reaction does not occur for this question. Submit Request Answer

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Write reaction showing how each of the buffers
would neutralize added NaOH.
HCHO2 and NaCHO2
Express your answer as a balanced chemical equation. Identify all of the phases in your answer.
0
ΑΣΦ
Submit
A chemical reaction does not occur for this question.
?
Request Answer

Part B
What is the [H3O+]?
Express your answer using one significant figure.
[H3O+] =
Submit
15| ΑΣΦ
Request Answer
?
M

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2) did i do this right?
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The following tabulated data is provided to answer this question and the remaining questions in the quiz. The post lab data will appear each page so that you can refer back to this data, as needed. Review the data, then answer the first question below. The equation is H2SO4 + NaOH → Na2SO4 + H20 (note, this equation is unbalanced) The last two rows are left blank because they will be filled in by your calculations. Titration Lab Trial 1 Trial 2 Trial 3 Volume of Acid Used 20.0 mL 20.2 mL 20.8 mL Molarity of Acid Used 0.05 M 0.05 M 0.05 M Initial Buret Reading 0.00 mL 0.00 mL 0.00 mL Final Buret Reading 20.7 mL 21.0 mL 21.5 mL Volume of NaOH Used Molarity of NaOH Solution What is the correct balanced equation for the neutralization reaction? Select one: O a. H2SO4 + NaOH → Na2SO4 + H2O O b. H2SO4 + 3 NaOH → Na2SO4 + 3 H2O c. H2SO4 + NaOH → Na2SO4 + 2 H20 O d. H2SO4 + 2 N2OH → N22SO4 + 2 H2O
Answer the questions by writing the correct letter of your answer. Explain your answer briefly in 1 or 2 When a strong acid is added to a non-buffered solution with a pH of 8, the pH of the solution decreases to a pH of 3. When the same strong acid is added to a buffered solution with a pH of 8, the pH of the solution will most likely a. increase b. decrease to pH 7 c. decrease to pH 3 d. remain at pH 8
Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components initial type (check all that apply) change effect of change on pH (check one) O acidic A H₂O, KOH basic ○ pH higher add KI O pH lower neutral acidic B H₂O basic add H CIO4 O neutral ☐ acidic C H₂O ☐ basic add Na CIO O neutral acidic O pH the same O pH higher O pH lower O pH the same O pH higher O pH lower O pH the same O pH higher D H₂O, KOH basic add HI O pH lower Oneutral O pH the same
I need help for number 5 part b and c
Each question in a paragraph?
Box 1 and 2. box 1 answer choices: higher, lower, or unchanged. box 2 answer choices: higher, lower, or unchanged.
Please provide only typed answer solution no handwritten solution needed allowed Please do it all instant positive rating
Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components initial type (check all that apply) change effect of change on pH (check one) acidic pH higher H₂O add HClO4 basic pH lower neutral pH the same acidic pH higher B H₂O, HBr basic add KOH pH lower neutral pH the same acidic pH higher с H₂O, HBr basic add K Br pH lower neutral pH the same acidic pH higher D H₂O basic add NaC104 pH lower neutral pH the same
4) Start with 800 ml 1.2M Acetic Acid, what would be the pH? How many grams of NaOH would it take to destroy only 28% of the acid? What would be the pH at that point?
Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. initial type (check all that apply) effect of change on pH (check one) solution initial components change acidic pH higher H,0 add HNO3 basic O pH lower neutral pH the same acidic O pH higher H,0, H Br add Na OH basic pH lower neutral pH the same acidic pH higher H,0 add KNO3 C basic pH lower neutral pH the same acidic pH higher H,0, H Br add Na Br basic pH lower neutral O pH the same O O 0O O 0 0 O C O000 000