# If 25 mL of 0.055 M HCl is added to 35 mL of distilled H2O, what is the final pH? A) 0.20 B) 1.26...

## Question:

If 25 mL of 0.055 M HCl is added to 35 mL of distilled {eq}H_2O {/eq}, what is the final pH?

A) 0.20

B) 1.26

C) 1.41

D) 1.64

## Strong Acids

Strong acids are acids that completely dissociate in water, producing a high concentration of hydrogen ions. Examples of strong acids include hydrochloric acid, sulfuric acid, and nitric acid.

## Answer and Explanation: 1

Become a Study.com member to unlock this answer! Create your account

View this answerOur first step is to calculate the final concentration of HCl using the dilution equation.

{eq}\rm C_2=\frac{C_1V_1}{V_2}=\frac{(0.055\ M)(25\...

See full answer below.

#### Ask a question

Our experts can answer your tough homework and study questions.

Ask a question Ask a question#### Search Answers

#### Learn more about this topic:

from

Chapter 11 / Lesson 9Learn about strong acid - strong base titration. Understand strong acid - strong base reactions and how to find an unknown substance concentration, and see the curve.

#### Related to this Question

- If 25 mL of 0.750 M HCl is added to 100 mL of 0.250 M NaOH, what is the final pH?
- What is the resulting pH of a solution when 25.00 mL of 0.1044 M NaClO2(aq) is titrated with 0.1078 M HCl after the following volume additions. a. 0 mL of HCl added b. 12.37 mL of HCl added c. 24.21 mL of HCl added d. 37.14 mL of HCl added
- 8.00 mL of 0.300 mol/L HCl solution is mixed with 12.0 mL of distilled water. Calculate the pH of the diluted solution.
- What is the pH when 46.00 mL of a 0.150 M NaOH solution have been added to 50.00 mL of a 0.130 M HCl solution?
- If exactly 50 mL of a 0.050M solution of hydrochloric acid is added to exactly 50 mL of 0.050M ammonia, what is the pH of the resulting solution?
- If 300 mL of 3.9 M HCl is added to 400 mL of 2.9 M NaOH, what is the pH? What is the concentration of NaCl in the resulting solution?
- If you add 0.50 ml of 0.10 M NaOH to 25.0 ml of distilled water and mix it, what will be the pH of the resulting solution?
- A 499 mL sample of 0.9038 M HI is mixed with a 527 mL sample of NaOH (pH of 13.65). What is the pH of the final solution?
- What is the hydronium ion concentration, (in M), in a final solution when 25 mL of 0.074 M HBr and 35 mL of 0.021 M \ HCl have been mixed together at 25^oC?
- Assuming complete dissociation, what is the pH of a 0.005 m HCl solution?
- What is the pH of a 1.23 x 10-3 M solution of HCl?
- The temperature for each solution is carried out at approximately 297 K, where Kw = 1.00 x 10-14. a. 0.10 g of hydrogen chloride (HCl) is dissolved in water to make 6.0 L of solution. What is the pH of the resulting hydrochloric acid solution? b. 0.60 g o
- A solution is prepared by adding 50.0 mL concentrated hydrochloric acid and 20.0 mL concentrated nitric acid to 300 mL water. More water is added until the final volume is 1.00 L. Calculate (H+), (OH-), and the pH for this solution.
- What is the pH of an aqueous solution of 300 mm HCL?
- What is the pH of a 0.20 m HCl solution?
- How to prepare a 1600-mL solution of pH 1.50 using concentrated 12 M HCl?
- What is the pH of a 0.20 mol/dm^3 solution of HCl?
- Calculate the pH of a solution of HCl, given the hydrogen ion concentration is 8.7 \times 10^{-9} M.
- What would be the molarity of a solution obtained when 50.0 mL of 3.00 M HCl acid solution is diluted with 70.0 mL of water?
- What are the pH and pOH of a solution of 2.0 M HCl, which ionizes completely?
- What is the pH of 0.1 mol L-1 HCl?
- You have 15.00 mL of a 0.150 M aqueous solution of the weak base NH3 (Kb = 1.79 x 10-5). This solution will be titrated with 0.150 M HCl. a. How many mL of acid must be added to reach the equivalence point? b. What is the pH of the solution before any aci
- Assume the pH of your deionized water solution is 7. Then use this pH to calculate what the pH should be after adding 0.10 M NaOH to 50 mL of water. \\ Expected pH after adding 1 mL of 0.10 M NaOH to water. [{Blank}] Expected pH after adding 6 mL of 0.10
- If a solution is at pH 4, how many hydrogen ions are present in a final solution ending up at pH 7?
- What is the hydronium ion concentration in a solution formed by combining 200 mL of 0.15 M HCl with 300 mL of 0.090 M NaOH at 25 degrees Celsius?
- HCl is a strong acid, which means nearly every molecule of HCl in solution has dissociated into one H^+ ion and one Cl^- ion. If an HCL solution is 1\times 10^-1 M and the hydrogen ion concentration is also 1\times 10^-1, then what is the pH of the soluti
- You are presented with 20 mL of an aqueous HCl solution in a conical flask. By titration (using a pH meter), 8 mL of 0.4 M NaOH is needed to neutralize the solution. (a) What pH reading will the neutralized solution give? (b) What is the molar concentrati
- 2.50 x 10^2 mL of an 8.0 M solution of the salt of a weak acid (NaD) is added to 2.50 x 10^2 mL of water. The K_a of the acid HD is 2.5 x 10^-9. What is the pH of the final solution?
- What quantity of NaOH must be added to 2 L of 8.5 M HCl to achieve a pH of 13?
- A chemist needs 225 mL of 5.33 M HCl. What volume of 11.0 M HCl must be dissolved in water to form this solution?
- What volume of distilled water is required to make a 10 mM solution of HCl, starting with 50 mg of solid HCl? (The molecular weight of HCl is 36.5 g/mol).
- Calculate the pH of the following solution: Solution prepared by diluting 41.0 mL of 8.4 x 10^2 M Ba(OH)2 to a volume of 305.0 mL . Express your answer using two decimal places.
- We have 500.0 mL of a buffer solution that is 0.661 M in NH3 and 0.341 M in NH4Cl. We add 500.0 mL of a 0.237 M HCl solution. The final volume is 1.0 L. The Kb value for NH3 is 1.8 x 10-5. What is the pH of the final solution?
- What volume of water must be added to 10 mL of a pH = 2.0 solution of HNO3 in order to change the pH to 4.0?
- What is the pH of 0.00042 M HCl?
- A sample of 0.0084 mol of HCl is dissolved in water to make a 1500 ml solution. Calculate the molarity of the HCl solution, the ~[H_3O^+], and the pH. For a strong acid such as HCl, the ~[H_3O^+] is the same as the molarity of the HCl solution. HCl (a
- Brenda calculates the hydrogen ion concentration of her hydrochloric acid solution as 0.098 M. What is the pH of this solution?
- What is the pH of a 0.01 M solution of hydrochloric acid?
- What is the pH of a 0.05 M solution of HCl? Explain why HCl and HCHO2 do not have the same pH when the concentration is the same (0.05 M).
- Analyte: 100.0 mL of 0.111 M KCN (K_a (HCN) = 4.9 \times 10^{-10}) Titrant: 0.100 M HCl Calculate (a) the equivalence volume, (b) the initial pH, (c) the pH after adding 50.0 mL titrant, (d) the pH at half-equivalence, and (e) the pH at equivalence.
- How would you prepare 10 mL of a 0.25 percent m/V HCl solution if 1 percent m/V HCl was available? How much 1 percent m/V HCl is needed? How much distilled water is used?
- What is the concentration of h+ in a 2.5 m HCL solution?
- 1a. What is the hydroxide ion concentration in a solution of HCl at 2.70 x 10^-3 mol/L? b. What is the hydronium ion concentration in a solution with [OH^-] = 1.60 x 10^-10 mol/L? c. In a solution, the [H_3O^+] = 3.50 x 10^-6 mol/L. What is the hydroxid
- What volume of a concentrated hydrochloric acid solution, which is 36.0% hydrochloric acid by mass and has a density of 1.179g/mL, should you use to make 5.00L of a hydrochloric acid solution with a pH of 1.8?
- A solution has a hydrogen ion concentration of 1 x 10^6 M. What is the pH?
- If it takes 75.00 mL of a 2.50 M HCl solution to neutralize 55.00 mL of base NaOH of unknown concentration. i.) Calculate the concentration of an unknown basic solution. ii.) Based on the molarity of the base, calculated above, what is the pH of the solut
- What is the pH of an aqueous solution with a hydrogen ion concentration of (H+) = 9.8 x 10-4 M?
- a. A solution has a hydrogen ion concentration of 6.3 \cdot 10^{ 10} \text{ M} . i. What is the pH of the solution? ii. What is the pOH of the solution? b. A weak acid dissociates according to the reaction \text{HA} \to \text{H}^+ + \text{A}^
- Calculate the pH and pOH of 12 M HCl.
- What is the pH of a solution prepared by adding 53.6 ml of 0.100 M sodium hydroxide to 66.6 ml of 0.897 M hypochlorous acid, HClO?
- Which of the following will result in a solution of 0.50 M HCl? A. 250mL of 2.0 M HCl added to 750 mL H2O B. 500 mL of 1.0M HCl added to 1,000 mL H2O C. 100 mL of 0.50 M HCl added ...
- Suppose 0.12 g of hydrogen chloride is dissolved in enough water to make 0.25 L of solution. Calculate the pH of the solution.
- Consider the titration of 50.00 mL of 0.1090 M brucine with 0.06150 M HCl. Calculate the pH at each of the following points: a. the initial point b. 50.00 mL c. the equivalence point
- Calculate the pH of 0.20mol dm^3 hydrochloric acid (HCl) and pH of 0.20 mol dm^3 of sulfuric acid (H2SO4).
- Which is the pH of a solution in which the concentration of hydrogen ion is greater than the concentration of hydroxide
- How many mm of water must be added to dilute 100mm of a 0.2mol/dm3 solution of HCl acid to a 0.01 solution?
- Calculate the pH of a 0.30 M HCl solution. How would the pH of a 0.30 M acetic acid solution compare to your calculated pH value for 0.30 M HCl?
- What is the concentration of an HCl solution if 25.0 mL of the solution is neutralized completely by 40.0 mL of a 0.30 M KOH solution?
- A solution of a strong acid has a pH of 3. What is the concentration of hydronium ions in this solution? (Hint:
- If 1 ml of 0.1 m NAOH is added to 1 L of the acid, what is the resulting pH?
- Consider the titration of 10 mL of 0.30 M pyridine (C5H5N; Kb = 1.7 x 10^-9) with 0.100 M HCl. Calculate: pH after 50.0 mL HCl added
- You are presented with 25 mL of an aqueous solution of HCl in a conical flask. A titration performed using a 0.4 M aqueous NaOH solution and a pH meter reveals that the titer volume required to neutralize the acid solution is 10 mL. a) Calculate the pH of
- 1.0 x 10-8 moles of HNO3 are added to 1.0 l of pure H2O. What is the pH?
- Consider the titration of 10 mL of 0.30 M pyridine (C5H5N; Kb = 1.7 x 10^-9) with 0.100 M HCl. Calculate: initial solution pH
- If 0.4 M HCl is added to an equal volume of 0.6 M NaOH, what are the new concentrations of OH- and H3O+?
- Which of the following will result in a solution of 0.50 M HCI? A. 250 mL of 2.0 M HCl added to 750 mL H_2O B. 500 mL of 1.0 M HCI added to 1,000 mL H_2O C. 100 mL of 0.50 M HCI added to 900 mL H_20 D. 200 mL of 0.10 M HCI added to 1,000 mL H_2O
- The hydrogen ion concentration is 1 ? 10^-7. What is the pH of this solution?
- Calculate the volume of acid and water needed to prepare 50 mL of each solution. a. Volume of HCl b. Volume of H2O
- If I had 0.280L of a 6.00M solution of HCl, and added enough water to lower the concentration to 4.50M, what would my new volume be?
- A buffer solution contains 0.408 M NaH2PO4 and 0.360 M K2HPO4. Determine the pH change when 0.104 mol HCl is added to 1.00 L of the buffer.
- Consider the titration of 30.0 mL of 0.259 M weak base B (Kb = 1.3 x 10) with 0.150 M HI. What would be the pH of the solution after the addition of 100.0 mL of HI?
- Consider the titration of 30.0 mL of 0.259 M weak base B (Kb = 1.3 x 10) with 0.150 M HI. What would be the pH of the solution after the addition of 20.0 mL of HI?
- Which of the following will result in a 0.5 M solution of HCl? a. 250 mL of 2.0 M HCl added to 750 mL water b. 500 mL of 1.0 M HCl added to 1,000 mL water c. 100 mL of 0.50 M HCl added to 900 mL water d. 200 mL of 0.10 M HCl added to 1,000 mL water Plea
- What is the hydrogen ion [H^+] concentration of a solution of pH 8?
- What is the pH of the solution at the equivalence point in the titration of 150 mL of 0.1 M ammonia with 0.1 M HCI? ''K%%(vertical-align: sub)a%%'' for NH4⁺ = 5.6 ×10⁻¹⁰.
- The molar concentration of H+ ions in a solution is 5.8 x 10-9. What is the pH?
- Calculate the pH of a solution that is prepared by adding 25.0 mL of a 0.20 M HBr solution to 15.0 mL of a 0.10 M KOH solution. Assume that the final volume is the sum of the two initial volumes.
- What is the pH of a solution with a (H+) of 5.73 x 10^-5?
- What is the concentration of OH in a solution of 0.5M HCl?
- Calculate the pH of a 0.25 M HCI solution. How would the pH of a 0.25 M acetic acid solution would compare to your calculate pH for the HCI solution?
- Given that the pH of a solution is 6.7, what is the [h3o+]?
- What is the pH of a solution that contains 2.31 x 10-6 M H3O+?
- What is the pH of a solution with [H3O+] = 1 x 10-9 M?
- What is the pH of a solution with [H3O+] = 1 x 10-9 m?
- What is the pH of a solution with H3O+ = 1.0 x 10-9 M?
- Would a 1.0?10-8 m solution of HCL have pH < 7, ph=7, or ph > 7?
- Determine the pH of the solution after the addition of 2.35 mL of 1.21 M cesium hydroxide (CsOH) to 48.40 mL of 0.982 M pyridinium chloride (C_5H_5NHCl).
- Calculate the hydrogen ion concentrations in each of the following solutions. a. pH = 1.05 b. pH = 5.65 c. pH = 2.42
- Calculate the pH of a solution obtained by mixing 100 ml 0.1 M HNO_2 with 400 ml 0.05 M KOH.
- Suppose 25.0 mL of a 0.212 M NaOH solution is neutralized by 13.6 mL of an HCl solution. What is the molarity of the HCl solution?
- The amino acid histidine is a triprotic acid with pK values of 1.8, 6.0 and 9.2. a. If you begin with a solution containing 10 mmol of His at pH 6.0, what will be the final pH after adding 10 mmol of HCl?
- A solution containing 4.75 g of calcium phenoxide (C6H5O)2Ca is diluted with water until it reaches a pH = 10.84. What is its final volume?
- How much of a 12.0 M HCl solution would you need to create 400 mL of a 0.25 M HCl solution?
- Calculate the pH of a 0.20 M NH₃ / 0.20 M NH₄Cl buffer after the addition of 10.0 mL of 0.10 M HCl to 65.0 mL of the buffer. Be sure your answer has the correct number of significant digits. (Note: Reference the __''K%%(vertical-align: sub)
- A solution has a pH of 11.60. What is the value of H+ for this solution?
- a. What is the pH of a solution that is 0.155 \text{ M} in dimethulamine and 0.135 \text{ M} in dimethylammonium ion? b. What is the Ph of a 250.0 \text{ mL} sample of the solution from part a agter the addition of 10.0 \text{ mL}
- Calculate the pH of a solution for which H+ = 1.0 x 10-3 M.
- The figure shows the pH titration curve of 0.100 \ M \ NaOH against 0.100 \ M \ HCl. To the nearest milliliter, what is the initial volume of HCl solution?
- What is the pH of 8? 10-8 m HCL?
- What is the ph of 8 x 10^-8 m HCl?