Five students, Ali, Bob, Chanda, Durga and Emmanuel, tested five different solution (one solution per student) separately with Universal Indicator showed pH as 4, 1, 11, 7 and 9 respectively. Whose solution is:
(i) Neutral (ii) Strongly alkaline (iii) Strongly acidic (iv) Weakly acidic (v) Weakly alkaline.p>
i> Neutral- Durga's solution is neutral (pH= 7)
ii> Strongly Alkaline- Chanda's solution is strongly alkaline (pH=11)
iii> Strongly Acidic- Bob's solution is strongly acidic (pH=1)
iv> Weakly Acidic - Ali's solution is weakly acidic (pH=4)
v> Weakly Alkaline- Emmanuel's solution is weakly alkaline ( pH=9)
(The pH of a solution is a measure of the molar concentration of hydrogen ions in the solution and as such is a measure of the acidity or basicity of the solution.
The letters pH stand for "power of hydrogen" and numerical value for pH is just the negative of the power of 10 of the molar concentration of H+ ions.
To calculate the pH of an aqueous solution you need to know the concentration of the hydronium ion in moles per litre (molarity).
The pH is then calculated using the expression: pH = - log [H3O+].
Related Articles
- Five solutions A, B, C, D, and E when tested with universal indicator showed pH as 4, 1, 11, 7, and 9 respectively. Which solution is?(i) Neutral?(ii) Strongly alkaline?(iii) Strongly acidic?(iv) Weakly acidic?(v) Weakly alkaline? Arrange the pH in increasing order of hydrogen-ion concentration.
- Two solutions X and Y have pH = 4 and pH = 8, respectively. Which solution will give alkaline reaction and which one acidic?
- Name an indicator which is pink in alkaline solution but turns colourless in acidic solution.
- Which is more acidic: a solution of pH = 2 or a solution of pH = 6?
- Explain the acidic solution and the basic solution.
- A solution changes the colour of turmeric indicator from yellow to red. The solution isbasicacidicneutral either neutral or acidic
- An aqueous solution ‘A’ turns phenolphthalein solution pink. On addition of an aqueous solution ‘B’ to ‘A’, the pink colour disappears. The following statement is true for solution ‘A’ and ‘B’.(a) A is strongly basic and B is a weak base.(b) A is strongly acidic and B is a weak acid.(c) A has pH greater than 7 and B has pH less than 7.(d) A has pH less than 7 and B has pH greater than 7.
- You have two solutions A and B. The pH of solution A is 6 and pH of solution B is 8.i. Which solution has more hydrogen ion concentration?ii. Which of this is acidic and which one is basic?
- (a) What effect does the concentration of H+ (aq) ions have on the nature of a solution?(b) What effect does the concentration of OH– ions have on the nature of a solution? (c) Someone put some universal indicator paper into vinegar. The pH is 3. What does this tell you about the vinegar? (d) Someone put some universal indicator paper onto wet soap. The pH is 8. What does this tell you about the soap? (e) State whether a solution is acidic, alkaline or neutral if its pH is :(i) 9 (ii) 4 (iii) 7 (iv) 1 (v) 10 (vi) 3
- Which is more basic (or more alkaline): a solution of pH = 8 or a solution of pH = 11?
- Fill in the following blanks with suitable words:(a) Acids have a pH ______ than 7.(b) Alkalis have a pH _____ than 7.(c) Neutral substances have a pH of _____.(d) The more acidic a solution, the _____ the pH.(e) The more alkaline a solution, the ______ the pH.
- Which one of the following solutions would you use to test the pH of a given sample?(1)blue litmus solution(2)red litmus solution(3) universal indicator solution(4)mixture of red and blue litmus solution
- On adding phenolphthalein indicator to colourless solution, no change is observed. What is the nature of this solution?(a) Basic(b) Either acidic or basic(c) Either acidic or neutral(d) Either basic or neutral
- A student measured the pH values of four solutions P, Q, R and S as 10, 6, 0 and 12 respectively. The solution which is the most acidic is likely to be the solution :(1) P (2) Q (3) R (4) S
Kickstart Your Career
Get certified by completing the course
Get Started
To Continue Learning Please Login
Login with Google